okay
welcome to uh lecture here
we'll get started here in just a second
go ahead and put here into the chat box
roll
so we're gonna continue on with chapter
10 and as you know we do have a quiz
today so what we're going to do
is uh we're going to lecture here for
just a little bit
we're going to stop early then you could
go take your quiz
on canvas using proctorial and then
we'll have lab
afterwards so we'll do a little bit of
lecturing again we'll
we'll stop here uh early probably a
little bit maybe around 11 15
or so and you'll use the rest of the
time there to go take your quiz
and afterwards we will have lab like
normal um during our normal sort of time
we may start just a little bit later in
terms of lab um but that's sort of the
plan so
a little bit of lecturing here up front
uh stopping early
quiz and then off to um
lab after that and i think that's uh
what we've got scheduled here for today
okay so
uh uh we've been talking about energy in
this last chapter here
um remember that you know energy
uh really a lot of times how we sort of
deal with it is to classify
what's happening in terms of energy as
really one of two things
either an exothermic type of process
where heat and energy is released are an
endothermic type process where heat and
energy is
absorbed and as we talked a little bit
about i think
last time as well if it's exothermic
what that essentially means when we look
at say something like a
energy diagram um that we saw earlier
that means that our reactants
are higher in energy than our products
so they have to give off energy which is
sort of an exothermic part of it
uh to get to the products and vice versa
for an endothermic our reactants are
lower in energy than our products so in
order to get up there to our products
has to put energy in
and again that's more of an endothermic
type process
and in terms of values as we'll see in
this chapter and i think as we talked
about as well
if something's sort of exothermic in
terms of heat and energy if you
calculate it
it will usually give you a negative
value in terms of the
value for energy if the process is more
endothermic when you actually calculate
which we'll do some of this here coming
up
you will get more of a positive number
so
there's two sort of values that we
commonly see that we'll talk about here
coming up
delta h which is the enthalpy again if
that
delta h value as we will see is a
positive number it means endothermic
if it's a negative number means
exothermic and q
which is basically heat or energy as
well uh we'll do some calculations for
that
and same deal if you get a negative
value for q that's going to be
exothermic and a positive value will be
endothermic
so i think where we left off was right
about here
we were talking about sort of energy
and the first law of thermodynamics and
thermodynamics in general
um basically deal with the ideas whether
or not under certain conditions
would we expect a reaction to occur and
uh
the first law of thermodynamics deals
with energy and it's the conservation of
energy
so we don't lose energy in any type of
process we don't gain energy in any type
of process
so there's sort of a conservation of
energy overall in the universe
but we do have that energy sort of
transferring from one place to the next
and again a lot of times when we think
about sort of what's happening
in terms of energy we think about in
terms of the system which is typically
whatever we're dealing with
and the surroundings which is typically
everything outside of that
so for example if you're doing a
reaction in a beaker uh the system would
be the beaker and then the surroundings
would be
everything pretty much outside of that
beaker
so a little bit about internal energy
and we don't really get into
a heck of a lot really on this on this
stuff here
but just to kind of cover it here the
change in internal energy which is delta
e
is equal to q plus w q again
here is heat so when we see this q value
here
represents heat and as you can see below
there w
represents work uh so a lot of times we
do use energy to do some type of work on
something
our work is being done on something else
and the change in internal energy
is the sum really of the kinetic and
potential energies
of a particle in a system again kinetic
energy is the energy due to motion
potential energy is the energy kind of
stored energy if you will
the energy due to sort of its position
and again that classic sort of example
of a big giant boulder on top of the
hill
has a certain amount of potential energy
uh it can't go over the hill and start
moving down which would transfer it to
kinetic energy
um so that's sort of what we're talking
about here same sort of convention here
with the e
in terms of energy the change in
internal energy again usually negative
means more of an
exothermic and positive means more
energy is being absorbed
endothermic type of representation
so again we talked a little bit about
this but just to reiterate uh
if we calculate q which a lot of times
in this class we will deal with mostly q
uh and when we do calculate q again that
positive value means endothermic
and that negative value means exothermic
and the idea here is as we talked about
for example
this system lost five joules of energy
it would be negative for the system as
it is exothermic
it's losing that energy when we talk
about sort of the surroundings out here
the surroundings would gain five joules
of energy in that sort of example
again here the actual value or number
will be the same
the only sort of difference here is the
sign to sort of reflect whether or not
the energy is being given off
or being absorbed and again this is sort
of that idea as well that conservation
of energy so
although the system lost that five
joules of energy
it wasn't completely lost and gone
forever it was absorbed by something
else in this case the surroundings would
gain that five joules of energy
so again for us you know we'll see q a
lot and
it's good to understand and have that
idea that the positive value
means endothermic absorbing energy
negative exothermic
in terms of work again we don't do a
heck of a lot with work in
in sort of this class you'll probably
cover it a little bit more in uh
what they call it classier 1a i think
but
the sign is well so work is basically
you know something that's being done
sort of force over distance and
same idea if the system is doing work on
the surroundings it's negative
almost sort of the same idea as
exothermic if it's releasing energy
being negative
and if work uh if the surroundings is
doing work on the system
it would be positive so the work sort of
being done on the system
as well and again sort of the same
classification so for us you know
probably worry about too much in terms
of work
or anything like that um
so in an endothermic process here again
uh
q would be heat and again for our
purposes q would be a
positive value and work is done on the
gas and the process is
exothermic so if work is being done
on the on the gas by the surroundings
then that would be positive for work
again if the process is exothermic then
the q value or the heat value would be
negative in that case
so
so let's talk about some important units
though uh when we do talk about
energy uh really uh there's two sort of
big units that we commonly come across
and these are them here
this is calories and joules and the
definition of a calorie
and one thing about this calorie is it
is actually a lowercase c
and that's important because there's
also another calorie that's a
capital c so you'll see calories as with
a capital c
and you'll see calories with a lowercase
c so
usually uh in chemistry here we usually
deal a lot with the lowercase calories
and a calorie is basically the amount of
heat that's required to change
one gram of water by one degree celsius
a joule is also another unit
of energy that's used a lot
also sort of the kilo versions of these
guys are also used a lot
uh kilocalories is used a lot a
kilocalorie is a
thousand of our little calories
also kilojoules is used a lot and that's
a thousand
of our joules so that's a very common
sort of
unit of that so what this calorie with
the capital c is is a nutritional
calorie
and basically one calorie with a capital
c
is the same as a thousand of the little
calories with the little c
and that's the same as one kilocalorie
so you know if you've ever been on like
a treadmill or anything like that
sometimes where they show the calories
they'll show how many kilocalories
you're burning
and again that's sort of a nutritional
calorie which is the capital c so
again the capital c does so usually
represent that nutritional calorie
so usually here we do really deal with
the
lowercase c and this conversion here you
do need to know
as the big arrow says i suppose this is
the conversion to go from calories
to joules and in one calorie there's
4.184
joules and that is definitely a
conversion that you use a lot uh in
chemistry especially
and what we're going to be talking about
here which is sort of specific heat
it's used a lot
so here if we wanted to convert 60.1
calories into joules we could use that
conversion factor to do so
we could use dimensional analysis as
well so here we would start with our
60.1
calories this is our conversion factor
that we just had
again the calories are going to cancel
each other out
going to leave us with joules and we end
up with 251 joules
again in terms of significant figures we
would be defaulting back to this guy
here
as this guy is a convergent factor here
so it's an exact number so we don't have
to worry about it
so here we have three significant
figures and
three sig figs on this guy here as well
and again that's a very common
conversion that you have to do a lot
especially when you're dealing with
things like specific heat and stuff like
that
going from calories to joules and joules
back to calories
now the uh the heat required to
change the temperature does depend on
the substance and the amount of the
substance or the number of grams
the temperature change and the identity
of the substance
and there's something as we will see
here in just a second which is known as
the specific heat capacity
and the specific heat capacity really is
that is is the amount of heat required
really to change
one gram of a substance by one degree
celsius
and that's why specific heat capacity as
we'll see i think on the next slide
perhaps
has units of joules per gram per degree
celsius
our common units are calories per gram
per degree celsius and again it's
basically the definition there the
energy
like joules required to raise one gram
of a substance
by one degree celsius so that's why it
has all three of these sort of units
associated with it
and again it is that amount of energy
that's required to
change that substance by one degree
celsius per one gram
that means if you think about it uh if
you have a larger value for the specific
heat capacity
of a substance it takes more energy to
convert
or change the temperature by one degree
than if you had somebody that had a
smaller one
so if you had somebody that had .25
joules per gram per degree celsius
versus somebody that has specific heat
capacity
of say 3.2 joules per gram per degree
celsius
it would take a lot more energy that
need to be put in there to change the
guy on the right there
by one degree celsius then it would the
the
substance there on the left in this made
up example again on the left you just
need to put in 0.25 joules of energy per
gram
um to raise it while the other one
you've got to put in about 3.2
so you could look at something like the
specific heat capacity of a substance
and it can kind of give you an idea as
to whether or not uh you know
you have to take a lot of energy to
change the temperature or not so for
example
water liquid water
so liquid water has a specific heat
capacity of 4.184
joules per gram per degree celsius hence
where that conversion comes from
and we also have one calorie per gram
per degree celsius
so this is specific heat capacity of
liquid water
and a reminder as well that what we will
see
in some of these examples is when you do
look up the
values these are typically values you
can find in a table you do want to look
it up for not only what you're looking
for in terms of the substance
but you do want to look it up in terms
of the actual state
and water is a very common one that you
come across as you need to look up
but for example if you had something
like ice which is also water
but as water in the solid state the
specific heat capacity for something
like ice is like 2
joules per gram per degree celsius so it
does change depending on the
state of it and again you'll see a table
i think we have one in here if not
you'll
see one in your book but you do want to
make sure that what you're looking up
for
is not only you know the right substance
but also the right state it's in solid
liquid or gas
when you go to that table and again
sometimes people just grab like the
first one they see in the table oh
that's water i'm not really sure what
state it's in but we'll just go with
that number
and you do want to make sure um that you
do get the right state
this is probably also some numbers here
the 4.184 and the one that you should
know
as well which is a specific heat of
water and like i said
that's one that's used a lot in
chemistry
and here is that table and as you can
see um
when we do water which is ice a very
different number
and even gas is actually a slightly
different number
so really important when you go to the
table like this that
again you take a look at the states of
those guys and make sure that you get it
we see some things like um some solids
over here we've got some silver
some gold has 0.24 and you can see on
this table
just looking at these values you can see
water has a
a pretty high specific heat capacity
and that's why it actually takes a lot
of heat to change water by one degree
celsius
which is why typically if we have a
pretty large body of water
um you know like our oceans and stuff
like that it you know
it takes a lot of energy to actually
change it by one degree celsius
and when you do start to see you know
the temperature for example of the ocean
and stuff like that change
by you know a degree celsius or two you
may think yourself doesn't seem like a
lot
but because water has a very high
specific heat capacity
to get water to change by even one
degree celsius means that there must be
a
lot of heat there to allow that to
happen and that's sort of the idea right
behind things like you know global
warming and stuff like that
all right so again uh calories as well
and i i would say also probably in most
cases though
uh we will see mainly joules
but you will see some problems involve
calories so
very common people are kind of used to
eating as joules but
calories as well does pop in there
and again as the big arrow says you do
need to know that value there of the
4.184
and the one calorie per gram per degree
celsius
and again that's specifically for liquid
water
now there is a forma that we use and
it's sometimes referred to as a specific
heat formula
and this is the formula that's used to
calculate the amount of heat required
you know to change a substance in terms
of its temperature
so this formula is used when we have a
substance that's in the same state
so for example it's liquid all the way
through but we decided to change the
temperature of it so you know we want to
take it from say 20 degrees celsius
to 60 degrees celsius all still the same
liquid in that
sort of area and this is q is equal to
ms
delta t the q here is heat or energy and
again it has typically units of joules
or calories depending on sort of
which one you're going with s is our
specific heat capacity which we were
just talking about and it has units of
either joules per gram for degrees
celsius
are again calories per gram degrees
celsius
depending on which one you're trying to
choose m is the mass
and it has units of grams as you can see
down there
and delta t is temperature
and this is one of the few uh formulas
in chemistry where
you actually do not need to change the
temperature to kelvin so you can
actually
usually leave it in degrees celsius but
it is in degrees celsius
and the reason it's in degree celsius is
pretty much our specific heat capacity
has degrees celsius so all the units
will cancel
now the important part about delta t
delta t is not just the temperature but
it's actually the
change in temperature
and what that really means is when you
do delta t
you want to take the final temperature
minus the initial temperature
now the truth is if you didn't take
final minus initial and you just took
the difference of the temperature
and you put all the numbers into this
equation you will get the same answer
for q
regardless of sort of if you did final
minus initial or just did larger minus
smaller
but it's really important to actually do
final minus initial and the reason for
that is
when we look at specific heat capacity
this is a positive number
when we look at the mass it is also a
positive number
which means what truly determines
what is going to happen in terms of q
and what i mean is will it be a negative
value or a positive value
is actually this part of it the change
in temperature
so if our temperature started at 20
degrees celsius
and went to 60 degrees celsius the
temperature increased
in order for the temperature to increase
you have to put heat and energy in
and then we will see a reflection of the
temperature go up
and that should be an endothermic
process and that means our q should be
positive so here if we did final
temperature
60 minus initial temperature 20
that gives us a change in temperature of
40 degrees which is
positive and we would end up with a
positive q
and as we've been talking about positive
q means endothermic
which is what we would expect now if the
opposite was true and our temperature
started at 60 degrees
and we threw it on ice and we ended at
20 degrees
when we do our change in temperature it
technically should be
20 minus 60 which gives us minus 40
degrees in this example
the minus part here because the rest of
these guys are positive we'll turn our q
into a negative number which means it
would be
exothermic which is also what we would
expect it to be in this situation
the only way the temperature could go
down is it has to release that heat and
energy
and it does go down so sometimes when
people are taught this equation they're
taught just take the larger number minus
the smaller number
which numerically speaking you will get
the same value
but it is really important to make sure
that you do the change in temperature as
final minus initial
because again that's going to give you
the correct sign
either positive or negative when you do
this equation
any questions on that there
so obviously this equation you do need
to know obviously how to use it
and let's take a look maybe an example
here
all right so why don't you take a second
here calculate the amount of heat and
energy
uh needed to raise the temperature of
6.25 grams of water
from 21 to 39 degrees celsius
see what you come up with
okay so uh here again we're going to use
really that q
is equal to ms delta t
we do have m given to us not given to us
which is
specific heat capacity here of liquid
water we're assuming
so remember that s is 4.184
joules per gram per degree celsius or
again it is one calorie per
degrees uh per degree per grams
um but here we are looking for joules so
we might as well obviously use
this version of it which means we do
have this and we do have our two
temperatures here
as well so obviously we just need to
plug it in
so our mass is 6.25 grams
our specific heat capacity joules per
gram per degree celsius
and again here we want to do our final
temperature which is
39 degrees celsius minus our initial
which is 21 degrees
celsius and if we do all that good stuff
there we do end up perhaps with
something like 471
and the units would be grams would
cancel degrees celsius would cancel
joules are the only unit that is left
there and we would end up with joules
here
any question on that particular one
there
and in terms of sort of sig figs uh
we're multiplying there so we got three
sig figs on that one
four and then actually when we take 39.0
minus 21.0
that's uh 18.0 technically the number
should be
which is also three significant figures
so probably should end up with three
significant figures when it's all said
and done
again ultimately the last thing that you
did was multiply all the way across
and everybody had two of them had three
sig figs and the guy in the middle there
had
four any questions on that particular
one
also we see that the temperature went
from 21 and
increase to 39 which would imply that
this should be
endothermic and we do see a
positive value here for q which also
tells us that it is endothermic so all
that does make sense
you know in terms of the sign and
everything that's going on with this one
all right so hopefully they agree with
me
that's a lot of slides to this example
there you go all right
so they they're rounded off they put the
little line but round it off to 471
it'll be fine
i try this one here a pure stamp of iron
requires 142 calories of energy
to raise the temperature from 23 to 92
what is the mass of the sample
specific heat capacity of iron is 0.45
so see what you come up with
okay so on this one again we're going to
use our
formula here q is equal to ms delta t
we have 145 calories and that would be q
142 calories we do have our
final and initial temperature initial
temperature being 23 degrees celsius
final temperature being 92 degrees
celsius
and we do have the specific heat
capacity given to us which was 0.45
joules per gram degrees celsius so we
just kind of uh
take off here we have these guys we need
to solve for mass
we do have a little bit of a conversion
problem here
our q is in calories and
our specific heat capacity here is in
joules
so we do have to do a conversion so you
could do either one you can convert to
specific heat capacity into calories if
you want
or you can convert the q into calories
so here i'm going to convert the q into
calories so that's 142 calories
and again there is uh 4.184
joules per calorie
and if we do that here
142 times 4.184
gives us something like uh 594
joules technically should go about three
sig figs on that if you want to keep a
digit there you can until the end
at this point we could solve for m m
would equal
q divided by s delta t
and in this case 594 joules we just
converted
our specific heat capacity which was in
joules so all that should work okay
and again here our change in temperature
should be our final minus our initial
so we're going to do a 92 minus
23 degrees celsius
so uh degrees celsius will cancel joules
will cancel
when we do the dividing the grams will
come up up and top there
and if we do that divide it by 0.45 and
divided by
92 minus 23.
looks like we should end up with
probably 19
grams in this case and again in terms of
sig figs
i kept the whole number there's like 0.1
whatever is on the joules but
technically this should be
three sig figs uh this guy is
two sig figs and i believe when you
subtract these guys here to the whole
number
you also end up with two sig figs so
two sig figs there on the answer at the
end
question on that
okay
all right so try one more here specific
capacity of lead is 0.13
how many calories of heat would be
required
to raise the temperature of 150 grams of
lead from 25 to 100 degrees celsius
yeah i've got a question yeah it was
just about the other one
um yeah so did you just switch the
formula around to get
to how to find mass yeah so uh so this
was like kind of the original formula up
here the
ms delta t so basically we want to solve
for m so we want to divide
the s and delta t to the other side
okay and then they cancel and then
you're left with what we got down here
all right thank you you're welcome
can you please show the next example
yeah so i can write it down thank you
so
okay so uh here again uh
using our q is equal to ms delta t
uh we do have our s given to us which is
our
0.13 joules per gram degrees celsius
we do have the m given to us which is
our 150 grams
and we do have here our initial
temperature and this guy here being
our final temperature so really we do
have everything sort of on this side
to calculate q so we could actually just
put it in there so
q would be 150 grams our specific heat
capacity 0.13
joules per gram degrees celsius again
doing our final minus our initial which
would be 100
minus 25 degrees celsius and if we do
all that good stuff there
uh 150 times 0.13
times 100 minus 25
and that gives us an answer of about
1462.5
and in terms of the units here celsius
cancels
grams cancel we're left with joules at
this point
in terms of sig figs just to think about
where we really should be on this number
uh this guy's got four significant
figures this guy's got
two significant figures and when we
subtract that that should be 75 which
would also be
two significant figures that technically
means that our answer
should end up right about here at two
significant figures
although we're not really looking for
joules either we're actually looking for
calories so if you like you can just
hang
on to that number for now do the
conversion
of 4.184 joules
uh per calorie and the joules here will
cancel
and if we do that we do end up with
something like
349.54
a whole bunch of numbers calories again
we still should end up probably at two
significant figures
so probably something like 350.
calories we want to kind of clean it up
at the end
if you kind of cleaned it up earlier
there you might get a slightly different
number
you'll get something like 350
9 calories if you sort of rounded this
guy really strictly to 1500
at that point and then did it you'll end
up with something like 359.
again most time you probably want to
just kind of carry the numbers to the
very end
and clean it up at the end but if you
did round
uh 1500 it probably would be okay if you
got the 359
which technically you then should round
to 360 i guess it would be
on that case i have a question um
is the isn't the final um
a hundred wouldn't wouldn't this be a
negative number
the final is a hundred but uh when you
do change in temperature it's final
minus initial
oh okay okay thank you
and it so we do get a positive number
for q here which is what we would expect
because it should be endothermic
because the temperature started at 25
and it raised 100
so the only really way to do that is to
put heat and energy in right so it will
raise the temperature
if it was opposite and we ended at 25
and started at 100
energy would have to be released and be
exothermic
in order for that to occur other
questions on this
yeah i've got one um so
are you able to just convert the 0.13
joules over grams to
calories that's another option you could
do that you could convert the uh
the joules per gram for degrees celsius
there the specific heat capacity into
calories and just
plug it in again probably with rounding
it should be and hopefully it's kind of
the same ballpark
under the final answer but you
absolutely could do that as well yeah
other questions
yeah so you would probably be okay if
you rounded that to 1500 and then
continue on with the 1500
i would be able to figure it out which
did and as long as the final answer
again
um if you did that 1500 and you got down
to the final answer you would have
something like 358.5
you have needed to round it out to two
significant figures and then you would
be fine
in terms of significant figures which i
guess would be 360 at that point
other questions on this particular one
okay so i think we're gonna do is we're
gonna stop here right now for lecture
and uh let's talk a little bit about uh
what's gonna go on now
uh the quiz is going to happen uh so in
just a couple minutes i'll make the quiz
available
up on canvas uh the quiz
will be on canvas so you'll take it
through canvas you will need a piece of
paper
to do some work and show some work so
you could get some partial credit just
in case something goes bad with the
answer
you could use a calculator again no
notes or anything like that
you do have to use proctorial so you do
that's just like the practice quiz
that means you have to use a computer a
webcam and obviously chrome with the
proctorial
extension in there if it asks you for a
code for the quiz
that means that something is not correct
you're not using a computer you're not
using uh
the proctorial or you're not using
chrome so it should not ask you for any
type of access code if it does it just
means
you know your thing is not set up right
so that's why we did the practice quiz
so hopefully you got that all worked out
and it shouldn't be a problem um a
reminder that
there is an end time for the quiz uh so
you if you start right when it's
available you should be fine in terms of
not running out of time
if for some reason you decide to wait
which you should not do
you should start as soon as is available
and the computer cuts you off i will not
reopen that quiz for you yes so
make sure you start it uh once you hit
submit
your quiz will be submitted so there's
only
one submit button at the very bottom so
only hit it when you're completely done
with the quiz
and then hit the submit button if you
hit it before you answer all the
questions you'll actually put a warning
up like are you sure you want to do this
and the answer should be probably no yes
um so
you do need to show work on problems
that say you need to show work for it
they're
clearly labeled and those should be uh
done on paper
which needs to be uploaded after you
submit the quiz
um it is in his own module yeah so
you'll see it'll call
like taking quiz one module it's a whole
thing
and um you will go to that module you
got to do it in order
so the first thing you have to do is
look at there's an academic honesty
agreement
you need to sign the academic honesty
agreement there's kind of an electronic
version of it
um you could either print it and sign it
the paper version or the electronic
version type in your initials good
enough
and then it will open up the quiz you
take the quiz using proctorial
once you're done taking the quiz you
need to submit your work
immediately after you submitted your
quiz if you wait too long to submit your
work
though you will not get any points for
those questions
it's not like submit your answers online
and then decide oh i remember how to do
that later
you will not get points so you need to
submit that immediately or you will get
zero on those things
and
other than that i think that's pretty
much everything
that you need to do whatever you need i
think should be on there you don't need
a periodic table so one was not provided
for you
if you need a periodic table you're
doing something wrong i think on this
quiz
so you don't definitely need one and
make sure that you do take it a reminder
that if you click away from the quiz
i want to do that but if you click away
from the quiz or you the quiz closes or
whatever
you can't log back on but a reminder
that the timer will not stop
so as soon as you hit start you know
make sure you're ready to take it
other than that any questions on that
again what you will see is in just a
second when we're done here
there will be a whole module um that
will open up and again you gotta kind of
go in order of faith that you have a
question or
yeah i did have a quick question is
there a specific way that you would like
us to
like face our camera for proctorio to
see us besides like facing our yeah
i i would appreciate it if you could
kind of do it uh that shows obviously
you and your work area if you could kind
of get that
you know so i could kind of see what's
going on in your work area as well
that would be perfect um so and also
kind of see you
as well so that kind of combination with
their your workspace and yourself
uh would be perfect and stuff like that
got it thank you thank you
other questions okay so in terms of lab
we do have lab today so what we're going
to do is we're going to start lab just a
little bit later we'll start at 12 15
give everybody a chance after they take
the quiz get up and walk around
all that and then we'll do lab 12 15
through the lab link um
and then uh so i think it's uh physical
chemical changes part one or something
like that is the experiment and we'll do
that experiment
uh at about 12 15 we'll log in for that
just give everybody a little chance to
not have to run from one thing to the
next and stuff like that any questions
on anything else before we go
i have a question so
what specifically like what sections are
going to be on the quiz or like what
formulas do we need to know
uh so like uh all the formulas there
that we uh talked about in
it's uh specifically i believe just uh
this is chapter
two i believe in this uh in this in your
book yeah chapter one was nothing so
it's all should be whatever we covered
in chapter two it's fair game
so i think only in chapter two you
pretty much had density i think was the
only formula i think maybe that you had
and a reminder that the temperature
conversions will not be given to you
and you need to know those guys as well
other questions
okay so uh give me about a minute or so
then it should be up there there'll be
an announcement that will come out on
canvas with a link
to link you to the quiz and then again
like i said you'll have to do the
academic honesty thing
there's a pdf file if you want you can
print and sign in and upload it
or if not you just need to go to the
next one which is the electronic version
where you can kind of sign it
that will open up the quiz and then that
will open up your um
you're uploading your work remember as
well one last thing that there are
different versions yes so like a normal
quiz don't have the right answers on the
wrong version or anything done like that
that's going to have to make me give you
a zero and your answers that you submit
online do you need to match the answers
that you upload
as well all right good luck on your quiz
and like i said in about a minute or so
you'll see an announcement through
canvas
and i'll have a link to it as whereas it
will be in the module section
and it will say something like taking
quiz number one and again i'll see
everybody
at 12 15 for lab to start
and if you didn't put here for the role
make sure you do that before you log off
you
