Consider the following reaction:A_{(g)} + 3 B | vedclass

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

Question

(B) The relationship between Gibbs free energy,enthalpy,and entropy is given by the equation: $\Delta G^{\ominus} = \Delta H^{\ominus} - T \Delta S^{\

Vedclass · Accepted Answer

$-50.33$

Vedclass · Answer

(B) The relationship between Gibbs free energy,enthalpy,and entropy is given by the equation: $\Delta G^{\ominus} = \Delta H^{\ominus} - T \Delta S^{\ominus}$.Given values are: $\Delta G^{\ominus} = -9 \ kJ = -9000 \ J$,$\Delta H^{\ominus} = -24 \ kJ = -24000 \ J$,and $T = 25 + 273 = 298 \ K$.Substituting these values into the equation: $-9000 = -24000 - (298 	imes \Delta S^{\ominus})$.Rearranging the terms: $298 	imes \Delta S^{\ominus} = -24000 + 9000 = -15000$.Solving for $\Delta S^{\ominus}$: $\Delta S^{\ominus} = -15000 / 298 \approx -50.33 \ J \ K^{-1}$.

Consider the following reaction:
$A_{(g)} + 3 B_{(g)} \longrightarrow 2 C_{(g)} ; \Delta H^{\ominus} = -24 \ kJ$.
At $25^{\circ} C$,if $\Delta G^{\ominus}$ of the reaction is $-9 \ kJ$,the standard entropy change (in $J \ K^{-1}$) of the same reaction at the same temperature is:

Similar Questions

For a spontaneous process,which of the following conditions is most favorable?

The relation between $\Delta G$ and $\Delta H$ is

For the vaporization of water at $1 \ atm$ pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ/mol$ and $108.8 \ J/K \cdot mol$ respectively. At what temperature $(K)$ will the change in Gibbs energy $(\Delta G)$ be zero (in $.4$)?

Under what conditions does a reaction always occur spontaneously?

For the spontaneity of a reaction,which statement is always true?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Consider the following reaction:$A_{(g)} + 3 B_{(g)} \longrightarrow 2 C_{(g)} ; \Delta H^{\ominus} = -24 \ kJ$.At $25^{\circ} C$,if $\Delta G^{\ominus}$ of the reaction is $-9 \ kJ$,the standard entropy change (in $J \ K^{-1}$) of the same reaction at the same temperature is: