QuestionApril 30, 2025

Determine Delta S for the phase change of 1.10 moles of water from solid to liquid at 0^circ C.(Delta H=6.01kJ/mol)

Determine Delta S for the phase change of 1.10 moles of water from solid to liquid at 0^circ C.(Delta H=6.01kJ/mol)
Determine Delta S for the phase change of 1.10 moles of water from solid to liquid at 0^circ C.(Delta H=6.01kJ/mol)

Solution
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Answer

\Delta S = 0.02421 \, \text{kJ/K} Explanation 1. Use the entropy change formula for phase transition The formula is \Delta S = \frac{\Delta H}{T}, where \Delta H is the enthalpy change and T is the temperature in Kelvin. 2. Convert temperature to Kelvin T = 0^{\circ}C + 273.15 = 273.15 \, K 3. Calculate \Delta S \Delta S = \frac{6.01 \, \text{kJ/mol}}{273.15 \, \text{K}} = 0.02201 \, \text{kJ/(mol·K)} 4. Multiply by moles Total \Delta S = 0.02201 \, \text{kJ/(mol·K)} \times 1.10 \, \text{mol} = 0.02421 \, \text{kJ/K}

Explanation

1. Use the entropy change formula for phase transition<br /> The formula is $\Delta S = \frac{\Delta H}{T}$, where $\Delta H$ is the enthalpy change and $T$ is the temperature in Kelvin.<br /><br />2. Convert temperature to Kelvin<br /> $T = 0^{\circ}C + 273.15 = 273.15 \, K$<br /><br />3. Calculate $\Delta S$<br /> $\Delta S = \frac{6.01 \, \text{kJ/mol}}{273.15 \, \text{K}} = 0.02201 \, \text{kJ/(mol·K)}$<br /><br />4. Multiply by moles<br /> Total $\Delta S = 0.02201 \, \text{kJ/(mol·K)} \times 1.10 \, \text{mol} = 0.02421 \, \text{kJ/K}$
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