General non-science questions and class announcements.

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

Celine Hoh 2L wrote:
Karyn Nguyen 1K wrote:For worksheet 4, is the answer for 6a wrong? I did (3/2)(31.9 mol)(8.314 J/Kmol)(311.15 K) = 124 kJ. When I didn't convert the temperature from C to K I got 15.1 kJ which is the answer given in the key.

We don’t have to convert it to kelvin as it is change in temperature (38-0)
Last edited by Karyn Nguyen 1K on Tue Feb 12, 2019 10:25 pm, edited 1 time in total.

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

Celine Hoh 2L wrote:
Karyn Nguyen 1K wrote:For worksheet 4, is the answer for 6a wrong? I did (3/2)(31.9 mol)(8.314 J/Kmol)(311.15 K) = 124 kJ. When I didn't convert the temperature from C to K I got 15.1 kJ which is the answer given in the key.

We don’t have to convert it to kelvin as it is change in temperature (38-0)

Don't we need to convert it to K to cancel out the units and end up with J?

ariana_apopei1K
Posts: 89
Joined: Fri Sep 28, 2018 12:27 am
Been upvoted: 1 time

Celine Hoh 2L wrote:Quick question for Worksheet 1 ques8:

When I2 is added, neither products nor reactants is favored as I2 is a solid.
What happens when I2 is removed, does the reaction not shift too?

Yeah, since it is a solid it doesn't affect it either way

Jane Burgan 1C
Posts: 73
Joined: Fri Sep 28, 2018 12:15 am

Karyn Nguyen 1K wrote:
Celine Hoh 2L wrote:
Karyn Nguyen 1K wrote:For worksheet 4, is the answer for 6a wrong? I did (3/2)(31.9 mol)(8.314 J/Kmol)(311.15 K) = 124 kJ. When I didn't convert the temperature from C to K I got 15.1 kJ which is the answer given in the key.

We don’t have to convert it to kelvin as it is change in temperature (38-0)

Don't we need to convert it to K to cancel out the units and end up with J?

We don't need to convert to K because the temperature difference in terms of celsius and in terms of kelvin are the same value.

Anjali_Kumar1F
Posts: 62
Joined: Fri Sep 28, 2018 12:25 am

Is there answer where it shows the work for these worksheets.

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

Anjali_Kumar1F wrote:Is there answer where it shows the work for these worksheets.

No, she only posts the answer key online, but during her workshop, she goes over how to do the problems!

Emily Huang 1E
Posts: 30
Joined: Fri Sep 28, 2018 12:20 am

Why is for delta H combustion, the equation is the the delta h combustion of reactants minus delta h combustion products whereas for delta h of formation it is the opposite?

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Hi students, there will be no workshop on Sunday because of the long weekend. Sessions will resume 2/24.

Enjoy the weekend after your midterm!

-K

Julia Lee
Posts: 80
Joined: Fri Sep 28, 2018 12:29 am

So is there no worksheet for this week?

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Julia Lee wrote:So is there no worksheet for this week?

No worksheet this week! The next session will cover all topics on Test 2.

Karina Jiayu Xu 4E
Posts: 58
Joined: Fri Sep 28, 2018 12:29 am

This is so helpful. Are the attachments basically study guides?

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

This week we will go over Gibbs free energy and most of electrochemistry (everything your test will cover). This is two sessions worth of material so please bear with me, see you there!
Attachments
Worksheet 7 - Electrochemistry .pdf
Worksheet 6 - Free Energy.pdf

Kobe_Wright
Posts: 83
Joined: Fri Sep 28, 2018 12:16 am

Thanks for the worksheet it helped a lot!

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Here are the keys to the Gibbs free and electrochem worksheets. As promised, for electrochem, I tried including as much detail as I can to follow through since there was not enough time to go over it.

NOTE:
For Gibbs free energy worksheet #3a, I made a mistake today in session saying that the conditions are at equilibrium. That is INCORRECT - the conditions are at standard conditions but not equilibrium. This follows through such that delta G at equilibrium is 0 and shouldn't be shifting to any side of the reaction. In 3a, it just so happens that P is 1, because 1/1^2 is 1, but P does not equal K (which is based on concentrations). So instead of writing RTlnK, I should've wrote RTlnP. Sorry for confusion.

If there are any other further confusions/mistakes, please let me know! I am still in the process of editing and perfecting these worksheets.
Attachments
electrochem worksheet W19.pdf
Worksheet 6 KEY - Free Energy.pdf

Julia Lee
Posts: 80
Joined: Fri Sep 28, 2018 12:29 am

Can someone please explain #4 on the electrochem worksheet? I don't understand why the answer is Ag+ not Fe2+

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

For the worksheet 7 (electrochem) question 2, I don't get why the E value would cause C to be false. Can someone explain this to me please?

Karyn Nguyen 1K
Posts: 72
Joined: Fri Apr 06, 2018 11:04 am

When we balance the equations on worksheet 7, how do we know which side of the reaction to add H2O to?

Vincent Li 4L
Posts: 48
Joined: Fri Sep 28, 2018 12:19 am

Julia Lee wrote:Can someone please explain #4 on the electrochem worksheet? I don't understand why the answer is Ag+ not Fe2+

Since you want copper to spontaneously reduce, then you need to check the oxidation values of elements/options given. In order to have a spontaneous reaction with copper reducing, the cell potential must be positive, so the oxidation potential of the substance must be positive, or the reduction potential of the substance must be negative. Fe2+ and Al3+ both work since they fulfill this criterion. I think the #4 answer just has an error.

Posts: 62
Joined: Fri Sep 28, 2018 12:26 am

On #1 of the Gibbs to find the standard enthalpy and entropy of formation you have to do the sum of products minus the sum of the reactants using the numbers given right? For some reason I am not getting the same answer.

Posts: 62
Joined: Fri Sep 28, 2018 12:26 am

In the Gibbs WS #4 how do you find T? or can you just assume its at 25 C?

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Vincent Li 4L wrote:
Julia Lee wrote:Can someone please explain #4 on the electrochem worksheet? I don't understand why the answer is Ag+ not Fe2+

Since you want copper to spontaneously reduce, then you need to check the oxidation values of elements/options given. In order to have a spontaneous reaction with copper reducing, the cell potential must be positive, so the oxidation potential of the substance must be positive, or the reduction potential of the substance must be negative. Fe2+ and Al3+ both work since they fulfill this criterion. I think the #4 answer just has an error.

Actually, when something says plain "copper" or "iron" use the actual solid and not the ion form (Cu2+, Fe3+, etc). With that said, because the question is asking for what can copper reduce, copper is acting as a reducing AGENT, which means it is oxidized, so we will use -0.52V for its oxidation potential. For reduction potentials, we leave as is on the chart. For Ag+, it is 0.80V. Total potential = reduction potential + oxidation potential, so 0.80 + (-0.52) leaves you with a positive potential value, which is what we want in order for a reaction to be spontaneous because delta G = -nFE. The values for the other ions, all have an absolute value less than 0.52 which would cause the total E to be negative, which is NON-spontaneous.

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Karyn Nguyen 1K wrote:For the worksheet 7 (electrochem) question 2, I don't get why the E value would cause C to be false. Can someone explain this to me please?

In order for a spontaneous reaction to occur, total E must be a positive value and when you add up the values for answer choice c, it is negative.

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Karyn Nguyen 1K wrote:When we balance the equations on worksheet 7, how do we know which side of the reaction to add H2O to?

Usually add H2O to the opposite side you added H+ or OH- in order to balance the number of O and H atoms

Shivangi_2J
Posts: 65
Joined: Fri Sep 28, 2018 12:15 am

on electrochem worksheet #8d, does it matter if on the cell diagram NO is listed first or NO3 is listed first? Or can the order of these two be reversed and the diagram still denotes the same reaction

Angela Grant 1D
Posts: 67
Joined: Fri Sep 28, 2018 12:25 am

Madison Hurst wrote:In the Gibbs WS #4 how do you find T? or can you just assume its at 25 C?

yeah you just assume 25 C, so 298 K

Angela Grant 1D
Posts: 67
Joined: Fri Sep 28, 2018 12:25 am

Madison Hurst wrote:On #1 of the Gibbs to find the standard enthalpy and entropy of formation you have to do the sum of products minus the sum of the reactants using the numbers given right? For some reason I am not getting the same answer.

the values are given per mole, are you multiplying them by the respective moles for each compound?
so delta H for example would be [-657.0 + 2(-110.5)] - [-910.0 + 2(0) + 2(0)] = 32 kJ/mol

Angela Grant 1D
Posts: 67
Joined: Fri Sep 28, 2018 12:25 am

for #4 on gibbs free energy, does it matter that the standard delta G is given in kJ instead of kJ/mol? i thought we'd have to divide by 2 to get the delta G per mole of NH3, but that didn't give me the right answer so i'm a little confused because plugging in the given value does give me the right answer even though it's not technically per mole

005199302
Posts: 108
Joined: Fri Sep 28, 2018 12:15 am

For #4 on the Gibbs worksheet, I keep getting -42.2 kj/mol and I can't figure out what I'm doing wrong

005199302
Posts: 108
Joined: Fri Sep 28, 2018 12:15 am

For #6 on the Gibbs free energy worksheet, how do we know that delta G is zero? Also, if delta G is zero and delta S of system is zero, why isn't delta S of surroundings also 0?

Samantha Ito 2E
Posts: 64
Joined: Fri Sep 28, 2018 12:29 am

Can someone please explain #4 on the Gibbs Free Energy worksheet?

Josephine Lu 4L
Posts: 62
Joined: Fri Sep 28, 2018 12:18 am

could someone please explain #8 part a on the electrochemistry worksheet? How do we know that S2O8 2- is reduced and NO is oxidized?

905084274
Posts: 42
Joined: Fri Sep 28, 2018 12:22 am

Did Karen post her most recent handout answer key that we weren't able to go over in session?

AhYeon_Kwon_2H
Posts: 48
Joined: Fri Sep 28, 2018 12:27 am

Could someone explain #3 on Worksheet 6? How would we find K without using partial pressure? Thanks!

AhYeon_Kwon_2H
Posts: 48
Joined: Fri Sep 28, 2018 12:27 am

Samantha Ito 2E wrote:Can someone please explain #4 on the Gibbs Free Energy worksheet?

I used deltaG = deltaGo + RTlnQ. I found Q with the pressure values that were given and assumed temperature to be 25oC, or 298K.

melissa_dis4K
Posts: 106
Joined: Fri Sep 28, 2018 12:28 am

Can someone pls explain how to calculate the equilibrium constant for Gibbs Free Energy wkst #1d? Thank you!

melissa_dis4K
Posts: 106
Joined: Fri Sep 28, 2018 12:28 am

Can someone pls explain how to do #3 from the Gibbs Free Energy worksheet.Thanks!

Fionna Shue 4L
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

For Worksheet 7 #8d, why is OH-(aq) not included in the cell diagram?

ariana_apopei1K
Posts: 89
Joined: Fri Sep 28, 2018 12:27 am
Been upvoted: 1 time

Josephine Lu 4L wrote:could someone please explain #8 part a on the electrochemistry worksheet? How do we know that S2O8 2- is reduced and NO is oxidized?

I also have this question

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

ariana_apopei1K wrote:
Josephine Lu 4L wrote:could someone please explain #8 part a on the electrochemistry worksheet? How do we know that S2O8 2- is reduced and NO is oxidized?

I also have this question

You look at the chart of reduction potentials. The one with the higher reduction potential will be reduced. For the other half reaction, it will become oxidized and all you need to do at that point is change the sign of the reduction potential for the half reaction that will become oxidized.

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Here is this week's worksheet focusing on reaction rates specifically differential rate law.
Attachments
Worksheet 8 - Kinetics Pt 1.pdf

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Key for differential rate laws.
Attachments
Worksheet 8 KEY - Kinetics Pt 1 .pdf

Julia Lee
Posts: 80
Joined: Fri Sep 28, 2018 12:29 am

Does anyone know if Karen posted worksheet 9 yet?

ariana_apopei1K
Posts: 89
Joined: Fri Sep 28, 2018 12:27 am
Been upvoted: 1 time

Julia Lee wrote:Does anyone know if Karen posted worksheet 9 yet?

no it would have been posted here, week 8 is the most recent

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Sorry for the delay in this week's worksheet! Didn't realize my last post didn't go through. This week we are reviewing integrated rate laws and if time permits, I will introduce reaction mechanisms. On Wednesday I will post a last worksheet for reaction mechanisms since I won't be seeing you next week due to your final on Sunday.

See you all tonight!
Attachments
Worksheet 9 - Kinetics Pt 2.pdf

Chem_Mod
Posts: 18880
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 714 times

Here is the key for last Sunday's worksheet and another worksheet focusing on reaction mechanisms. Full solutions are also given.

Good luck on your final!!!!!! It has been a great quarter!

Best,
K
Attachments
14B Mechanisms Worksheet Key.pdf
Worksheet 10 - Mechanisms.pdf
Worksheet 9 KEY - Kinetics Pt 2.pdf

CHEM 14B Lover
Posts: 33
Joined: Fri Sep 28, 2018 12:19 am

Thank you :)

annabel 2A
Posts: 67
Joined: Fri Sep 28, 2018 12:18 am

For the integrated rate law worksheet #5a, I found the answer using
1/((7.0*10^9 M*s)*(120 sec) + 1/0.086M)
= 1/ (8.4*10^11 M*s^2 + 11.63 M^-1)
and I got the right answer but I'm confused by the units. How do the units work out to be M? And how do you add 8.4*10^11 M*s^2 with 11.63 M^-1?

Josephine Lu 4L
Posts: 62
Joined: Fri Sep 28, 2018 12:18 am

### writing rate laws: "rate"or "d[A]/dt?"

when we write the rate laws, do we write it as "rate=..." or ""d[A]/dt=..."? Specifically in question #3 of the Reaction Mechanisms worksheet, could we replace "d[F]/dt" with "rate"?

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

For worksheet 8 #4d I am getting 144 M/s instead of 140 M/s. Am I doing something wrong?

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

How do you do #8 on worksheet 9? I tried to do .99[A]=.5^n[A] and solving for n by ln(.99)/ln(.5)=n, but this didn't work.

Semi Yoon
Posts: 60
Joined: Fri Sep 28, 2018 12:27 am

On Worksheet 9, how would you solve for #7?

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

Semi Yoon wrote:On Worksheet 9, how would you solve for #7?

For a first order reaction, you can use the equation (1/2)^n=whatever fraction of A is left because the half life is constant throughout the reaction. For this problem, use (1/2)^n=1/8 which means n is 3 (n is the number of half lives). We know the length of each half life is 355 seconds so the total time taken is 3x355=1065 s

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

### Re: writing rate laws: "rate"or "d[A]/dt?"

Josephine Lu 4L wrote:when we write the rate laws, do we write it as "rate=..." or ""d[A]/dt=..."? Specifically in question #3 of the Reaction Mechanisms worksheet, could we replace "d[F]/dt" with "rate"?

Yes they are synonymous. Writing it as d[A]/dt is just better because it specifies which species we are referring to.

Vincent Li 4L
Posts: 48
Joined: Fri Sep 28, 2018 12:19 am

Why is it that in #3 in the reaction mechanisms worksheet we're able to use the pre-equilibrium assumption to substitute and replace [C]? Wouldn't the approximation fail since the first and second steps are both fast, so there's no bottleneck to stop [C] form being consumed instead of forming A and B again?

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

Celine Hoh 2L wrote:Quick question for Worksheet 1 ques8:

When I2 is added, neither products nor reactants is favored as I2 is a solid.
What happens when I2 is removed, does the reaction not shift too?

Yes! Because it is a solid it is not included in the equilibrium equation so any change in concentration would not affect the reaction.

Emily Tam 1k
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

for number 5 of karen's 9th worksheet (kinetics), it says that the rate constant is 7.0x10^0 M.s. Does M stand for molarity or for minutes?

Emily Tam 1k
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

for number 6 of karen's 8th worksheet (kinetics pt 1),

why does k not depend on the order of the reaction? wouldn't the reaction order depend on the value of K?
If there is a higher order then wouldn't the k value be higher?

Emily Tam 1k
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

how do you solve 5a on worksheet number 9?
I know the second order equation is 1/[A]=kt+1/[A]0. If I were to use this equation, wouldn't I just plug the values given into the equation?
The answer that i got was 7.14x10^-11, which is different from the answer. pls help thxxxx

Emily Tam 1k
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

how do you solve for worksheet 9 number 6?

I used the half-life equation for a first-order reaction and solved for k when the half-life was 6 days.
my k value was 0.1155.
In order to find the percent of Hg(II) left in the body, would I have to find the k value for the 30-day half-life and divide the two k's?

Katie_Duong_1D
Posts: 69
Joined: Fri Sep 28, 2018 12:27 am

can someone please explain how to get the equilibrium constant for 1d in Gibbs free energy/worksheet 6? I keep getting 1.014.

Katie_Duong_1D
Posts: 69
Joined: Fri Sep 28, 2018 12:27 am

Katie_Duong_1D wrote:can someone please explain how to get the equilibrium constant for 1d in Gibbs free energy/worksheet 6? I keep getting 1.014.

I forgot to convert delta G from kj/mol to j/mol to match units. Now I get the correct answer 1.663 x 10^6.

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

Emily Tam 1k wrote:for number 5 of karen's 9th worksheet (kinetics), it says that the rate constant is 7.0x10^0 M.s. Does M stand for molarity or for minutes?

M stands for molarity, or mol/L

sonalivij
Posts: 70
Joined: Fri Sep 28, 2018 12:27 am

Emily Tam 1k wrote:how do you solve for worksheet 9 number 6?

I used the half-life equation for a first-order reaction and solved for k when the half-life was 6 days.
my k value was 0.1155.
In order to find the percent of Hg(II) left in the body, would I have to find the k value for the 30-day half-life and divide the two k's?

For first order reactions you can use the equation (1/2)^n=whatever fraction of A is remaining, with n being the number of half lives, since the half life is constant throughout the reaction. In this case we know 5 half lives would have passed (30/6=5), so we do 1/2^5 which yields 1/32 (3.1%) which means 3.1% of A is left after 30 days.

Shally Li 2C
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

sonalivij wrote:For worksheet 8 #4d I am getting 144 M/s instead of 140 M/s. Am I doing something wrong?

She rounded to 140 because you need to have two sig figs.

Jane Burgan 1C
Posts: 73
Joined: Fri Sep 28, 2018 12:15 am

how would you solve for worksheet 10 number 2 part c and d?

riddhiduggal
Posts: 30
Joined: Fri Sep 28, 2018 12:21 am

Amy Dinh 1A wrote:On #4a Worksheet 2, I keep getting pH=4.40, while the answer key says 4.30, when both using the quadratic formula and the shortcut way. I don't understand how to get the answer to

The pH is 4.40

abbydouglas1K
Posts: 65
Joined: Fri Sep 28, 2018 12:26 am

005199302 wrote:
ariana_apopei1K wrote:
005199302 wrote:For the first law worksheet, how do you do #2?

First you have to do stoichiometry to find how many moles of Pb is made from 49.7 g PbO. You multiply the number of moles of product times the enthalpy value given, which gives you the q to plug into your regular q=mCs(Tf-Ti). Once you solve for mass you should get the right answer

Which value should Cs be?

it should be the specific heat capacity for water but you must convert it to kilojoules

abbydouglas1K
Posts: 65
Joined: Fri Sep 28, 2018 12:26 am

Karyn Nguyen 1K wrote:
Celine Hoh 2L wrote:
Karyn Nguyen 1K wrote:For worksheet 4, is the answer for 6a wrong? I did (3/2)(31.9 mol)(8.314 J/Kmol)(311.15 K) = 124 kJ. When I didn't convert the temperature from C to K I got 15.1 kJ which is the answer given in the key.

We don’t have to convert it to kelvin as it is change in temperature (38-0)

Why do we use that equation for the change in internal energy and not q+w

Carissa Young 1K
Posts: 65
Joined: Fri Sep 28, 2018 12:17 am

How do you solve #8 on worksheet 9? How do you find the half-life given that 99% of the reactant decomposes in 137 min?

Ashley P 4I
Posts: 64
Joined: Wed Nov 15, 2017 3:04 am

Is there any worksheets for kinetics?

Ashley P 4I
Posts: 64
Joined: Wed Nov 15, 2017 3:04 am

Ashley P 4I wrote:Is there any worksheets for kinetics?

Nevemind I just found them, thank you for your help! Do you by chance have a final practice test? Or does anyone else have one?

rkang00
Posts: 69
Joined: Fri Sep 28, 2018 12:25 am

For the electrochem worksheet 8d, why don't we include the OH- in the cell diagram?

BenJohnson1H
Posts: 68
Joined: Fri Sep 28, 2018 12:17 am

Yes, it is further up in this thread and there is a key as well. There's also two parts!

abbydouglas1K
Posts: 65
Joined: Fri Sep 28, 2018 12:26 am

Chem_Mod wrote:
ariana_apopei1K wrote:
Josephine Lu 4L wrote:could someone please explain #8 part a on the electrochemistry worksheet? How do we know that S2O8 2- is reduced and NO is oxidized?

I also have this question

You look at the chart of reduction potentials. The one with the higher reduction potential will be reduced. For the other half reaction, it will become oxidized and all you need to do at that point is change the sign of the reduction potential for the half reaction that will become oxidized.

Thank you !!!

Lisa Werner 2F
Posts: 72
Joined: Fri Sep 28, 2018 12:17 am

in worksheet 5 problem 6, how do we know that work is 0?

Lisa Werner 2F
Posts: 72
Joined: Fri Sep 28, 2018 12:17 am

thank you so much karen! these worksheets were so helpful!

Posts: 62
Joined: Fri Sep 28, 2018 12:26 am

For kinetics ws pt 1 number 5 why isn't C included in the rate law? Is it an intermediate? if so, how can you tell?

Claudia Luong 4K
Posts: 59
Joined: Fri Sep 28, 2018 12:25 am

For worksheet 4 #6, I get a different value for the amount of work done. I get 12.4 kJ instead of 10.1kJ. Is there a mistake in the solutions?

AhYeon_Kwon_2H
Posts: 48
Joined: Fri Sep 28, 2018 12:27 am

Sorry, can someone explain worksheet 4 number 5 to me? Thank you!

Simmi Diwanji 2B
Posts: 32
Joined: Fri Sep 28, 2018 12:20 am

Thank you!

### Who is online

Users browsing this forum: No registered users and 1 guest