Water gas, a mixture of H₂ and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. a. Write the expression for the equilibrium constant for the reversible reaction: C(s) + H₂O(g) = CO(g) + H₂(g) AH 131.30 kJ b. What will happen to the concentration of each reactant and product at equilibrium if more C is added? c. What will happen to the concentration of each reactant and product at equilibrium if H₂O is removed? d. What will happen to the concentration of each reactant and product at equilibrium if CO is added? e. What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?

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**Water Gas Production and Equilibrium Analysis**

**Overview:**
Water gas, a mixture of H₂ and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon.

**Questions and Exercises:**

a. **Write the expression for the equilibrium constant for the reversible reaction:**

\[ \text{C (s) + H₂O (g) ⇌ CO (g) + H₂ (g)} \quad ΔH = 131.30 \text{ kJ} \]

b. **What will happen to the concentration of each reactant and product at equilibrium if more C is added?**

*Adding more C (solid) will not affect the equilibrium concentrations of the reactants and products in the gaseous phase because the concentration of a pure solid does not appear in the expression for the equilibrium constant.*

c. **What will happen to the concentration of each reactant and product at equilibrium if H₂O is removed?**

*Removing H₂O (g) will cause the equilibrium to shift to the left, favoring the formation of reactants to replace the removed H₂O (g).*

d. **What will happen to the concentration of each reactant and product at equilibrium if CO is added?**

*Adding CO (g) will shift the equilibrium to the left, favoring the formation of reactants to counteract the added CO (g).*

e. **What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?**

*Since the reaction is endothermic (ΔH is positive), increasing the temperature will shift the equilibrium to the right, favoring the formation of products CO (g) and H₂ (g).*
Transcribed Image Text:**Water Gas Production and Equilibrium Analysis** **Overview:** Water gas, a mixture of H₂ and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. **Questions and Exercises:** a. **Write the expression for the equilibrium constant for the reversible reaction:** \[ \text{C (s) + H₂O (g) ⇌ CO (g) + H₂ (g)} \quad ΔH = 131.30 \text{ kJ} \] b. **What will happen to the concentration of each reactant and product at equilibrium if more C is added?** *Adding more C (solid) will not affect the equilibrium concentrations of the reactants and products in the gaseous phase because the concentration of a pure solid does not appear in the expression for the equilibrium constant.* c. **What will happen to the concentration of each reactant and product at equilibrium if H₂O is removed?** *Removing H₂O (g) will cause the equilibrium to shift to the left, favoring the formation of reactants to replace the removed H₂O (g).* d. **What will happen to the concentration of each reactant and product at equilibrium if CO is added?** *Adding CO (g) will shift the equilibrium to the left, favoring the formation of reactants to counteract the added CO (g).* e. **What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?** *Since the reaction is endothermic (ΔH is positive), increasing the temperature will shift the equilibrium to the right, favoring the formation of products CO (g) and H₂ (g).*
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