ammonia is added to a gaseous reaction mixture containing H2, Cl2, and HCl that is at chemical equilibrium. How will the addition of ammonia affect concentrations of H2, Cl2, and HCl if the equilibrium constant of reaction two is much greater than the equilibrium constant of reaction 1?

Reaction 1- H2(g) + Cl2(g)---> 2HCl (g)

Reaction 2- 2HCl(g)+ NH3(g)---> NH4Cl(g)

Will reaction shift right, shift left, or will it have no effect?

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Jean KeelingLv2

13 Dec 2019

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1. Consider this reaction at equilibrium:

2 BrNO (g) <---> 2 NO (g) + Br2 (g)

Predict whether the reaction shift left, shift right, or remain unchanged after each disturbance. Explain in terms of reaction rates and collisions.

a. NO is added to the reaction mixture

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c. Br2 is removed from the reaction mixture

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Consider this reaction at equilibrium:

C (s) + H2O (g) <---> CO (g) + H2 (g)

Predict whether the reaction will shift left, shift right, or remained unchange after each disturbance. Explain.

a. C is added to the reaction mixture

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H₂ (g) + Cl₂ (g) -------> 2 HCl (g)
Appendix 4: H2 (g): âH^o = 0, âS^o = 131 J/K * mol, âG^o = 0. Cl2 (g): âH^o = 0, âS^o = 223 J/K * mol, âG^o = 0. HCl (g): âH^o = -92 Kj/mol, âS^o = 187 J/K * mol, âG^o = -95 Kj/mol

a) Calculate âH^o, âS^o, âG^o and equilibrium constant K (at 298 K) using data in Appendix 4 of Zumdahl textbook

b) If H₂ (g), Cl₂ (g), and HCl (g) are placed in a flask such that the pressure of each gas is 1 atm, in which direction will the system will shift to reach equilibrium at 25^oC?

Explain please.
Thanks!