For a reaction Delta H = 9.08 kJ mol^{-1} a | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) The reaction is endothermic because $\Delta H > 0$ $(9.08 \ kJ \ mol^{-1})$.To determine spontaneity,we use the Gibbs free energy equation: $\Delt

Vedclass · Accepted Answer

Spontaneous and Endothermic

Vedclass · Answer

(C) The reaction is endothermic because $\Delta H > 0$ $(9.08 \ kJ \ mol^{-1})$.To determine spontaneity,we use the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$.For the reaction to be spontaneous,$\Delta G$ must be negative $(\Delta G $\Delta G = 9080 \ J \ mol^{-1} - T(35.7 \ J \ K^{-1} \ mol^{-1})$.Setting $\Delta G  254.34 \ K$.Since the reaction can be spontaneous at temperatures above $254.34 \ K$ and is endothermic,option $(C)$ is the most appropriate description.

For a reaction $\Delta H = 9.08 \ kJ \ mol^{-1}$ and $\Delta S = 35.7 \ J \ K^{-1} \ mol^{-1}$. Which of the following statements is correct for the reaction?

Similar Questions

Assertion: Many endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature.
Reason: Entropy of the system increases with increase in temperature.

What is the nature of the reaction at $298 \ K$,if the entropy change and enthalpy change for a chemical reaction are $7.4 \ cal \ K^{-1}$ and $-2.5 \times 10^3 \ cal$,respectively?

Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.

For a certain reaction, $\Delta H^0 = -345 \text{ kJ}$ and $\Delta S^0 = -123 \text{ JK}^{-1}$. At what temperature will the change over from spontaneous to non-spontaneous occur (in $\text{ K}$)?

Which of the following reactions is expected to never be spontaneous?

Vedclass Test Series

Exam Paper Generator

Online Exam Module