Question

Zinc granules react with dilute $HCl$ to give $H_2$ at ${17}^{o}C$. The enthalpy change for the reaction is $-12.55kJ{mol}^{-1}$ and the entropy change equals to $5.0{JK}^{-1}{mol}^{-1}$. The Gibbs free energy change (in $kJ{mol}^{-1}$ ) of the reaction is $x$ , then magnitude of x i.e., $|x|$ is:

Answer 1

Given:

$\Delta H=-12.55kJmo{l}^{-1}$
$\Delta S=-5J{K}^{-1}mo{l}^{-1}$ and T= 17+ 273 = 290 K
$\Delta G=\Delta H-T\Delta S$
putting all the given values we get,
$\Delta G=x=-14kJmo{l}^{-1}$
$|x|=14$