Please help me with the following question. Please include all work and the corr

Question

Please help me with the following question. Please include all work and the correct answer in order to be rated.

Consider the reaction below: +198 kJ All of the following changes would shift the equilibrium to the left except one. Which one would not cause the equilibrium to shift to the left? (Circle the correct answer) a removing some SO3 b. decreasing the temperature c. ncreasing the container volume d. adding some so2 b. For which of the following reactions is Kc equal to Kp? (Circle the correct answer) a. 204(g) 2NO2(g) 2SO3(g) 2SO2 (g) O2 (g) d. C(s) CO2 (g) 2CO(g)

Explanation / Answer

1) the equilibrium will shift in such a way so that it may nullify the effect of stress applied to the system (Le-Chatelier's principle)

Given: reaction is endothermic (enthalpy is positive)

a) removing SO3: removing reactant from mixture shifts the reaction backward (left side)

b) decreasing temperature : The decrease in temperature shifts the endothermic reaction backward (left ), the side where heat will be evolved inspite of consuption

c) the increase in container volume will decrease the concentration.

The decrease in concentration will be compensated by shift of equilbrium towards the side where number of moles are more

in the given equilibrium the number of moles of gas of products > number of moles of gas of reactants

So the equilibrium will shift towards products(right)

This option is the answer: c

d) adding some SO2 will shift equilbirum towards product side (left)

b) We know that

Kp = Kc (RT)ng

R = gas constant

T = Temperature

ng = number of gaseous moles in products - number of gaseous moles in reactant

a) N2O4 --> 2NO2

Here ng > 0

so Kp > Kc

b) 2SO3 --> 2SO2 + O2

ng>0

Kp> Kc

c) H2 + Cl2 + 2HCL

ng = 0

Kp = Kc(RT)^0 = Kc

d) C + CO2 --> 2CO

ng > 1

Kp > Kc

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