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Consider a chemical reaction \mathrm{2 X+Y \rightarrow Z} at a certain temperature. The standard enthalpy change \mathrm{\left(\Delta H^{\circ}\right)} for the reaction is \mathrm{-200 \mathrm{~kJ} / \mathrm{mol}}, and the standard entropy change \mathrm{\left(\Delta S^{\circ}\right)\: is \: 150 \mathrm{~J} /(\mathrm{mol} \mathrm{K})}. Calculate the standard Gibbs free energy change \mathrm{\left(\Delta G^{\circ}\right)} for the reaction.
 

Option: 1

-244700 \mathrm{~J} / \mathrm{mol}

 


Option: 2

-54700 \mathrm{~J} / \mathrm{mol}
 


Option: 3

-242300 \mathrm{~J} / \mathrm{mol}
 


Option: 4

-230 \mathrm{~kJ} / \mathrm{mol}


Answers (1)

best_answer

Given data:
Standard enthalpy change \mathrm{\left(\Delta H^{\circ}\right)=-200 \mathrm{~kJ} / \mathrm{mol}}
Standard entropy change \mathrm{\left(\Delta S^{\circ}\right)=150 \mathrm{~J} /(\mathrm{mol} \mathrm{K})}
The standard Gibbs free energy change \mathrm{\left(\Delta G^{\circ}\right)} for the reaction can be calculated using the equation:
\mathrm{ \Delta G^{\circ}=\Delta H^{\circ}-T \Delta S^{\circ} }
Substitute the given values and calculate \mathrm{ \Delta G^{\circ} \text { : } }

\mathrm{ \Delta G^{\circ}=\left(-200 \times 10^3 \mathrm{~J} / \mathrm{mol}\right)-(298 \mathrm{~K}) \cdot(150 \mathrm{~J} /(\mathrm{mol} \mathrm{K})) \approx-200 \times 10^3 \mathrm{~J} / \mathrm{mol}-44700 \mathrm{~J} / \mathrm{mol} \approx-244700 \mathrm{~J} / \mathrm{mol} }

Therefore, the standard Gibbs free energy change \mathrm{\left(\Delta G^{\circ}\right)} for the reaction is approximately \mathrm{-244700 \mathrm{~J} / \mathrm{mol}.}

So, the correct option is 1.

Posted by

Gaurav

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