Consider the following equilibrium:
NH₄Cl(s)
NH₃(g) + HCl(g)
Suppose a vessel containing NH₄Cl(s) ,NH₃(g) and HCl(g) is at equilibrium.If the volume of the vessel is instantaneously doubled while keeping the temperature constant,when a new equilibrium is reached,which of the following statements is incorrect?

Question

Consider the following equilibrium:
NH₄Cl(s)

Consider the following equilibrium: NH<sub>4</sub>Cl(s) NH<sub>3</sub>(g) + HCl(g) Suppose a vessel containing NH<sub>4</sub>Cl(s) ,NH<sub>3</sub>(g) and HCl(g) is at equilibrium.If the volume of the vessel is instantaneously doubled while keeping the temperature constant,when a new equilibrium is reached,which of the following statements is incorrect? A) The value of K<sub>p</sub> remains unchanged. B) The number of moles of NH<sub>4</sub>Cl decreases. C) The total pressure is halved. D) The partial pressures of NH<sub>3</sub> and HCl in the vessel remain unchanged. E) The amount of NH<sub>3</sub> and HCl doubles.

NH₃(g) + HCl(g)
Suppose a vessel containing NH₄Cl(s) ,NH₃(g) and HCl(g) is at equilibrium.If the volume of the vessel is instantaneously doubled while keeping the temperature constant,when a new equilibrium is reached,which of the following statements is incorrect?

Quizplus · Accepted Answer

The Answer of Consider the following equilibrium: NH₄Cl(s) NH₃(g)+ HCl(g) Suppose a vessel containing NH₄Cl(s),NH₃(g)and HCl(g)is at equilibrium.If the volume of the vessel is instantaneously doubled while keeping the temperature constant,when a new equilibrium is reached,which of the following statements is incorrect?

Consider the Following Equilibrium