Sunday
September 21, 2014

Homework Help: Chemistry

Posted by Lisa on Sunday, February 10, 2013 at 4:32pm.

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 vessel is instantaneously doubled while keeping the temp constant when a new equilibrium is reacted, which of the following statements is correct?

A) the amount of NH3 and HCl double
B) the partial pressure of NH3 and HCl in the vessel remain unchanged
or

C) the total pressure is halved

I am going with B) because I think that the partial pressure will be unchange because of the solid in the equation. Is this correct?

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