(A) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,i.e.,$\Delta G < 0$.Given the equation $\Delta G = \Delt

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(A) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,i.e.,$\Delta G Given the equation $\Delta G = \Delta H - T\Delta S Convert $\Delta H$ to Joules: $\Delta H = -84.2 \ kJ = -84200 \ J$.Substituting the values: $-84200 \ J - T(-200 \ J \ K^{-1}) $-84200 + 200T $200T $T $T Thus,the highest temperature at which the reaction proceeds in the forward direction is $421 \ K$.

Class 11 Chemistry Thermodynamics Free energy and Work

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For a reaction $A + B \rightarrow$ products,$\Delta H = -84.2 \ kJ$ and $\Delta S = -200 \ J \ K^{-1}$. Calculate the highest value of temperature (in $K$) so that the reaction will proceed in the forward direction.

MHT CET 2023 All MHT CET

A
$421$
B
$237$
C
$168$
D
$273$

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For a reaction $A + B \rightarrow$ products,$\Delta H = -84.2 \ kJ$ and $\Delta S = -200 \ J \ K^{-1}$. Calculate the highest value of temperature (in $K$) so that the reaction will proceed in the forward direction.

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Calculate the work done in Joules $(J)$ when $50 \ g$ of iron is dissolved in $HCl$ in an open beaker at $25 \ ^oC$. The atmospheric pressure is $1 \ atm$.

For the reaction $x + y \rightarrow z$,the process is spontaneous at room temperature,and the reverse reaction is spontaneous at high temperature. Which of the following is true?

For a reaction at $25 \, ^oC$,the enthalpy change and entropy change are $-11.7 \times 10^3 \, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} \, K^{-1}$ respectively. What is the Gibbs free energy in $kJ$?

$2 \, mol$ of zinc is dissolved in $HCl$ at $25 \, ^oC$. What is the work done in an open vessel?

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