# Problem: 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.

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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.

What scientific concept do you need to know in order to solve this problem?

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Based on our data, we think this problem is relevant for Professor Halpin & Geggier's class at NYU.