For the hydrolysis of ATP at \(25^{\circ} \mathrm{C}(298 \mathrm{K})\) and
\(\mathrm{pH} 7, \mathrm{ATP}+\mathrm{H}_{2} \mathrm{O} \rightarrow
\mathrm{ADP}+\mathrm{P}_{1}+\mathrm{H}^{+},\) the standard free energy of
hydrolysis \(\left(\Delta G^{\circ}\right)\) is \(-30.5 \mathrm{kJ}
\mathrm{mol}^{-1}\left(-7.3 \mathrm{kcal} \mathrm{mol}^{-1}\right),\) and the
standard enthalpy change \(\left(\Delta H^{\circ \prime}\right)\) is \(-20.1
\mathrm{kJ} \mathrm{mol}^{-1}\left(-4.8 \mathrm{kcal}
\mathrm{mol}^{-1}\right)\) Calculate the standard entropy change \(\left(\Delta
S^{\circ}\right)\) for the reaction, in both joules and calories. Why is the
positive sign of the answer to be expected in view of the nature of the
reaction? Hint: You may want to review some material from Chapter 1.