TS EAMCET · Chemistry · Thermodynamics (C)
In the reaction \(\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{s})\) at \(0^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm}\), the internal energy change is \(-41 \mathrm{~kJ} / \mathrm{mol}\). What will be the value of molar enthalpy change?
- A \(-41 \mathrm{~kJ} / \mathrm{mol}\)
- B \(41 \mathrm{~kJ} / \mathrm{mol}\)
- C \(30 \mathrm{~kJ} / \mathrm{mol}\)
- D \(-30 \mathrm{~kJ} / \mathrm{mol}\)
Answer & Solution
Correct Answer
(A) \(-41 \mathrm{~kJ} / \mathrm{mol}\)
Step-by-step Solution
Detailed explanation
\(\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{s})\) at \(0^{\circ} \mathrm{C}, 1 \mathrm{~atm}\) This process of phase change from liquid to solid happens at constant temperature and pressure. So the change in internal energy will be the molar…
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