# Chemistry

Question: Consider following equilibrium system: SO2(g)+ Cl2(g) goes to So2Cl2(g) Kp=.900 atm @25 degree C. Suppose that 2.0 moles S02, 1.0 moles Cl2, and 3.0 moles So2Cl2 are placed in an empty 4.00L vessel at 25 degree C. Compute the number of grams of each substance present at equilibrium.

I set up an ICE table and converted all the moles of each substance to Molarity of each. Once i did that i got stuck, because the Kp is in atm and the other values are in molarity. What do i have to do to get atm of each and than convert those into grams?

1. 👍 0
2. 👎 0
3. 👁 265
1. You can change Kp to Kc.

1. 👍 0
2. 👎 0
posted by DrBob222
2. How do you change Kp to Kc?

1. 👍 0
2. 👎 0
posted by eliz
3. Kc = Kp(RT)^-delta n where
delta n = n(gas products) - n(gas reactants)

1. 👍 0
2. 👎 0
posted by DrBob222

I first changed Kp to Kc: .900atm(0.0821)(25+273.15)^(2.0 mol*1.0 mol)- (3.0)= 22.03

Than i did an ICE table. I than used the equation Kc= So2Cl2/So2*Cl2. 22.03=(.75+x)/(.5-x)(.25-x). I than solved for x. x=.169 was the only value that worked for x. I than substitued those into the each values to get moles than i changed them into grams of each. for the So2 I go 21.21g, for the Cl2 i got 5.74g and the SO2Cl2 i got 78.41 g. Is the correct way to do this problem?

1. 👍 0
2. 👎 0
posted by eliz
5. I didn't check the problem itself. I first checked the conversion of Kp to Kc.
First, you misunderstood the delta n part. The number of moles product n is 1 (its the coefficient, not the moles in the problem) and n for reactants is 2 (1+1)(again, not the values in the problem but the coefficients). Also, you turned it around; it should be products-reactants or 1-2=-1 BUT the good news is that your two errors canceled out and you came out with the right answer of -1. However, you did NOT include R within the parentheses so that makes your 22 incorrect.
I have Kc = Kp(RT)^-1 =
0.9/(0.08205*298.15) = about 0.04 but check my math. The 0.04 needs to be exact and not estimated on my part.

For the problem, you next need to determine which way the reaction is going in order to reach equilibrium.
SO2 + Cl2 ==> SO2Cl2
reaction quotient = (SO2Cl2)/(SO2)(Cl2) =
0.75/(0.5)(0.25) = 6.00
Since 6.00 is so much larger than 0.04, the reaction, as set up, is too far to the right so we know it will be shifting to the left.
Thus SO2 = 0.5+x; Cl2 = 0.25+x; SO2Cl2 = 0.75-x
and go from there.

1. 👍 0
2. 👎 0
posted by DrBob222

## Similar Questions

1. ### Chemistry

A gaseous reaction mixture contains SO2, Cl2, and SO2Cl2 in a 2 L container with the gases having the following partial pressures: P(SO2)=0.35 atm, P(SO2Cl2)=0.19 atm, P(Cl2)=0.24 atm. Kp=91 for the equilibrium system: SO2 (g) +

asked by Hannah on February 18, 2007
2. ### Chem

Hi! I need help with this question: Sulfur dioxide reacts with chlorine at 227 oC: SO2(g) +Cl2(g) ↔ SO2Cl2(g) Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction

asked by Anonymous on February 20, 2013
3. ### chemestry

At 100 °C the reaction: SO2Cl2(g) ⇄ SO2(g) + Cl2(g) has Kp = 2.4. Calculate the equilibrium composition of the mixture when 1.2 atm of SO2Cl2 are mixed with 0.8 atm of Cl2 at 100 °C.

asked by Anonymous on June 19, 2016
4. ### Equilibrium constant

Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A solution is made containing initial [SO2Cl2]= 0.022M . At equilibrium, [Cl2]= 1.7×10−2M Calculate the value of the equilibrium constant.

asked by Chemistry on May 5, 2015
5. ### chemistry

SO2Cl2(g) SO2(g) + Cl2(g) The Kp for the reaction is 2.18 at 648 K. A sample of SO2Cl2 is placed in a container and heated to 648 K while the total pressure is kept constant at 9.00 atm. Calculate the partial pressures of the

asked by helly on December 2, 2013
6. ### chemistry kinetics

The reaction SO2Cl2(g) → SO2(g) + Cl2(g) is a first order reaction carried out at constant volume at 600 K whose t1/2 is 4.1 hr. The initial pressure of SO2Cl2 is 1.25 atm. What will be the total pressure of the system after 1

asked by swa on May 24, 2012
7. ### chemistry

Please help me with this question For the system, (the previous post i forgot to post the Kp) PCl5 (g) --> PCl3 (g) + Cl2 (g) In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows:

asked by Jack on March 9, 2008
8. ### Chemistry

Sulfur dioxide reacts with chlorine at 227 oC: SO2(g) +Cl2(g) ↔ SO2Cl2(g) Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction vessel. After 15 minutes, the

asked by JOhn Boku on February 22, 2015
9. ### Chemistry

Use the data in the table to determine how long it will take for half of the original amount of SO2Cl2 to decompose at the average reaction rate. Experimental Data for SO2Cl2(g) → SO2(g) + Cl2(g) Time (min) [SO2Cl2](M) [SO2](M)

asked by Chloe on August 7, 2015
10. ### chemistry

Sulfuryl chloride, SO2Cl2, decomposes to SO2 and Cl2 according to the reaction SO2Cl2(g) -> SO2(g) + Cl2(g) The reaction is first order in SO2Cl2, and the value of the rate constant, k, is 2.20*10-5 /s at 300K. (a) Calculate the

asked by ssss on May 31, 2013

More Similar Questions