Consider the following equilibrium: 4NO(g) + 6H2O(g) 4NH3(g) + SO2(g); H > 0 Wha

ID: 983167 • Letter: C

Question

Consider the following equilibrium:

4NO(g) + 6H2O(g) 4NH3(g) + SO2(g); H > 0

What would you expect to happen if the temperature of the reaction vessel was lowered?

A. The partial pressure of H2O would decrease because the equilibrium would shift to the right

B. The partial pressure of NH3 would increase because the equilibrium would shift to the left

C. The partial pressure of NO would increase because the equilibrium would shift to the left

D. The partial pressure of SO2 would increase because the equilibrium would shift to the right

E. The partial pressures will all remain the same as lowering the temperature will not affect the equilibrium position

For the endothermic reaction

If the temperature of the reaction vessel was lowered,

C. The partial pressure of NO would increase because the equilibrium would shift to the left

Less heat supplied with lower temperature, will result in reversal of reaction, more starting material will be formed.

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