The equilibrium constant for the reaction
NH4Cl(s) → NH3(g) + HCl(g)
is 1.1 × 10−16 at 25°C. If the equilibrium constant is 6.5 × 10 −2 at 300°C, which statement is correct?
a) This is an enthalpy-driven reaction.
b) The reaction is spontaneous at high temperatures.
c) The reaction is spontaneous at all temperatures.
d) The reaction is exothermic.
e) The reaction is not spontaneous at any temperature.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Spontaneous Reaction concept. You can view video lessons to learn Spontaneous Reaction. Or if you need more Spontaneous Reaction practice, you can also practice Spontaneous Reaction practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofThe equilibrium constant for the reaction NH4Cl(s) → NH3(g)...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Jules took 3 minutes and 10 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Halpin & Geggier's class at NYU.