Problem: H2(g) is an important fuel source for hydrogen powered vehicles and a reagent for the Haber-Bosch process. A majority of H2 is generated using equilibrium below. C(s) + H2O(g) ⇌ CO(g) + H2(g)    ΔH°=131kJ/mol a) Write an equilibrium expression for this reaction.   b) predict the direction the equilibrium shifts (circle one) as a result of: 1. adding H2     left/reactants   right/products no change 2. removing CO   left/reactants   right/product  no change 3. adding more C left/reactants   right/product  no change 4. increasing temperature left/reactants   right/product  no change 5. increasing the pressure (by decreasing the volume) left/reactants   right/product  no change 6. increasing the pressure (by adding H2O) left/reactants   right/product  no change c) Which of the above disturbance/stresses/"pokes" will change the equilibrium constant (K)? Why? If none write "none".    

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H2(g) is an important fuel source for hydrogen powered vehicles and a reagent for the Haber-Bosch process. A majority of H2 is generated using equilibrium below.

C(s) + H2O(g) ⇌ CO(g) + H2(g)    ΔH°=131kJ/mol

a) Write an equilibrium expression for this reaction.

b) predict the direction the equilibrium shifts (circle one) as a result of:

1. adding H2    
left/reactants   right/products no change

2. removing CO  
left/reactants   right/product  no change

3. adding more C
left/reactants   right/product  no change

4. increasing temperature
left/reactants   right/product  no change

5. increasing the pressure (by decreasing the volume)
left/reactants   right/product  no change

6. increasing the pressure (by adding H2O)
left/reactants   right/product  no change

c) Which of the above disturbance/stresses/"pokes" will change the equilibrium constant (K)? Why? If none write "none".

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