Question

PQ-24. For the reaction $NH_4Cl(s) \rightleftharpoons NH_3(g) + HCl(g)$ $\Delta H^\circ = 176 \text{ kJ} \cdot mol^{-1}$ and $\Delta G^\circ = 91.2 \text{ kJ} \cdot mol^{-1}$ at 298 K. What is the value of $\Delta G$ at 1000 K? (A) -109 kJ·mol?¹ (B) -64 kJ·mol?¹ (C) 64 kJ·mol?¹ (D) 109 kJ·mol?¹

          PQ-24. For the reaction
$NH_4Cl(s) \rightleftharpoons NH_3(g) + HCl(g)$
$\Delta H^\circ = 176 \text{ kJ} \cdot mol^{-1}$ and $\Delta G^\circ = 91.2 \text{ kJ} \cdot mol^{-1}$ at 298 K. What is the value of $\Delta G$ at 1000 K?
(A) -109 kJ·mol?¹
(B) -64 kJ·mol?¹
(C) 64 kJ·mol?¹
(D) 109 kJ·mol?¹

PQ-24. For the reaction
NH4Cl(s) ⇌ NH3(g) + HCl(g)
Δ H^∘ = 176 kJ· mol^-1 and Δ G^∘ = 91.2 kJ· mol^-1 at 298 K. What is the value of Δ G at 1000 K?
(A) -109 kJ·mol?¹
(B) -64 kJ·mol?¹
(C) 64 kJ·mol?¹
(D) 109 kJ·mol?¹

Added by Noelia H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ajay Singhal

08/07/2021

Step 1

Step 1: Use the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, T is the temperature in Kelvin, and ΔS is the entropy change. Show more…

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PQ-24. For the reaction NH4Cl(s)⇌NH3(g)+HCl(g) ΔH∘=176 kJ⋅mol^(-1) and ΔG∘=91.2 kJ⋅mol^(-1) at 298K. What is the value of ΔG at 1000K? (A) -109 kJ⋅mol^(-1) (B) -64 kJ⋅mol^(-1) (C) 64 kJ⋅mol^(-1) (D) 109 kJ⋅mol^(-1)