# Consider the following reaction at equilibrium: NiO(s)+CO(g) 2 Ni(s) + CO2(g). Select all of the following...  Consider the following reaction at equilibrium: NiO(s)+CO(g) 2 Ni(s) + CO2(g). Select all of the following that will shift the reaction to the left side. Addition of CO Removal of CO Addition of Ni Increase the volume. Removal of CO2 Addition of CO2 Removal of NIO
Question 1 What is the expression for equilibrium constant for the following reaction? 2 H2S(g) + SO2(g) = 35(s) + 2 H2O(g) Kc= [HQ][S] [SO][H251 Kc= [HO] [H,872 Kc=  [H2 51 (H20 Kc= [H20] [51 (S02] [H282 Kc= [H0 [SO][251

--> kc = [CO2]/[CO]

Adding of CO will shift reaction towards right.

Removal of CO will shift reaction towards left.

Adding of Ni will have no effect.

Increase in volume will shift reaction towards more no. of gaseous molecules. So here, both side gaseous moles are equal hence no effect.

Removal of CO2 will shift reaction towards right.

Addition of CO2 will shift reaction towards left.

Removal of NiO will have no effect.

Option 2 and 6 will shift reaction towards left.

--> reaction is--

2H2S(g) + SO2(g) --> 3S(s) + 2H2O(g)

Kc = [H2O]2/[H2S]2[SO2]

Option 2.

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