1) Consider the reaction between sulfur dioxide and nitrogen dioxide: SO2(g) + N
ID: 824692 • Letter: 1
Question
1) Consider the reaction between sulfur dioxide and nitrogen dioxide: SO2(g) + NO2(g) <=====> SO3(g) + NO(g) Kc = 8.8 at 1000K
Given the following concentrations, predict in which direction the reaction will proceed:
a. [SO2 ] = 64.0 M, [NO2 ]=12.4 M, [SO3 ]=18.5 M, [NO ]=87.5 M
b. [SO2 ] = 1.73 M, [NO2 ]=0.581 M, [SO3 ]=4.89 M, [NO ]=158.2 M
c. PSO2 = 4.87 atm, PNO2 =4.87 atm, PSO3 =10.4 atm, PNO ]=10.4 atm
2) Consider the reaction:
HC2H3O2(aq) + H3O^+(aq) + C2H3O2^- (aq) Kc = 1.8e-5 at 25 deg C.
If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O^+ at 25 deg C.
3) Consider the following reaction:
Br2(g) + Cl2(g) <=====> 2BrCl(g) Kp= 1.11e-4 at 150K
A reaction mixture initially contains a Br2 partial pressure of 755 torr and a Cl2 partial pressure of 735 torr at 150K. Calculate the equilibrium partial pressure of BrCl.
Explanation / Answer
1. For the reaction:
SO2 (g) +N02 (g) ? SO3 (g) +NO (g)
KC=8.8
a. Here reaction quotient Q=[SO3][NO]/[SO2][NO2]
=18.5*87.5/64.0*12.4
=2.04
As Q< K, reaction will proceed in forward direction.
b. Here reaction quotient Q=[SO3][NO]/[SO2][NO2]
=4.89*158.2/1.73*0.581
=769.6
As Q> K, reaction will proceed in backward direction.
c. Now, Kp=Kc*(RT)?n
As ?n=0, for the above reaction
Kp=8.8
Here reaction quotient Q=PSO3*PNO/PSO2*PNO2
=10.4*10.4/4.87*4.87
=4.56
As Q< K, reaction will proceed in forward direction.
2. For the reaction
HC2H3O2? H3O+ +C2H3O2-
Initially: 0.210M 0 0
Finally: 0.210-x X X
KC=1.8*10-5
KC=[H3O+][C2H3O2-]/[ HC2H3O2]
1.8*10-5=X*X/(0.210-X)
Solving, X=1.935*10-3
So eqillibrium conc of H3O-=1.935*10-3M
3. For the reaction
Br2(g) + Cl2(g)? 2BrCl
Initially: 755 735 0
Finally: 755-X 735-X 2X
KP=1.11*10-4
KP=PBrCl2/PBr2*PCl2
1.11*10-4=(2X)2/(755-X)(735-X)
1.11*10-4(X2-1490X+554925)=4X2
Solving, X=3.90
So eqillibrium Pressure of BrCl=2X=2*3.90=7.80torr
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