Ethanol (C2H5OH)(C2H5OH) melts at --114 .C.C and boils at 78 .C.C. The enthalpy of fusion of ethanol is 5.02 kJ/molkJ/mol, and its enthalpy of vaporization is 38.56 kJ/molkJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g:KJ/(g:K), respectively. How much heat is required to convert 46.0 g of ethanol at -152 °C to the vapor phase at 78 °C? Express your answer in kilojoules to two significant figures. 15. ΑΣΦ kJ How much heat is required to convert 46.0 g of ethanol at 34 °C to the vapor phase at 78 °C? Express your answer in kilojoules to three significant figures. —| ΑΣΦ ? kJ
Ethanol (C2H5OH)(C2H5OH) melts at --114 .C.C and boils at 78 .C.C. The enthalpy of fusion of ethanol is 5.02 kJ/molkJ/mol, and its enthalpy of vaporization is 38.56 kJ/molkJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g:KJ/(g:K), respectively. How much heat is required to convert 46.0 g of ethanol at -152 °C to the vapor phase at 78 °C? Express your answer in kilojoules to two significant figures. 15. ΑΣΦ kJ How much heat is required to convert 46.0 g of ethanol at 34 °C to the vapor phase at 78 °C? Express your answer in kilojoules to three significant figures. —| ΑΣΦ ? kJ
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![**Ethanol Properties and Heat Calculations**
Ethanol \((\text{C}_2\text{H}_5\text{OH})\) melts at \(-114 \, ^\circ \text{C}\) and boils at \(78 \, ^\circ \text{C}\). The enthalpy of fusion of ethanol is \(5.02 \, \text{kJ/mol}\), and its enthalpy of vaporization is \(38.56 \, \text{kJ/mol}\). The specific heat of solid and liquid ethanol are \(0.97 \, \text{J/(g} \cdot \text{K)}\) and \(2.3 \, \text{J/(g} \cdot \text{K)}\), respectively.
**Problem 1: Calculate Heat Required**
1. **Scenario**: Determine the heat required to convert \(46.0 \, \text{g}\) of ethanol from \(-152 \, ^\circ \text{C}\) to the vapor phase at \(78 \, ^\circ \text{C}\).
- Express your answer in kilojoules to two significant figures.
\[
Q = \underline{\hspace{3cm}} \, \text{kJ}
\]
2. **Scenario**: Determine the heat required to convert \(46.0 \, \text{g}\) of ethanol from \(34 \, ^\circ \text{C}\) to the vapor phase at \(78 \, ^\circ \text{C}\).
- Express your answer in kilojoules to three significant figures.
\[
Q = \underline{\hspace{3cm}} \, \text{kJ}
\]
Note: This calculation involves multiple steps including heating the ethanol, phase changes, and using specific heat capacities.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb45a7b7-d1aa-4ac7-ad98-90aa0325071f%2F080a6a38-e031-4aac-852b-150946f7c282%2Fqqt0e6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Ethanol Properties and Heat Calculations**
Ethanol \((\text{C}_2\text{H}_5\text{OH})\) melts at \(-114 \, ^\circ \text{C}\) and boils at \(78 \, ^\circ \text{C}\). The enthalpy of fusion of ethanol is \(5.02 \, \text{kJ/mol}\), and its enthalpy of vaporization is \(38.56 \, \text{kJ/mol}\). The specific heat of solid and liquid ethanol are \(0.97 \, \text{J/(g} \cdot \text{K)}\) and \(2.3 \, \text{J/(g} \cdot \text{K)}\), respectively.
**Problem 1: Calculate Heat Required**
1. **Scenario**: Determine the heat required to convert \(46.0 \, \text{g}\) of ethanol from \(-152 \, ^\circ \text{C}\) to the vapor phase at \(78 \, ^\circ \text{C}\).
- Express your answer in kilojoules to two significant figures.
\[
Q = \underline{\hspace{3cm}} \, \text{kJ}
\]
2. **Scenario**: Determine the heat required to convert \(46.0 \, \text{g}\) of ethanol from \(34 \, ^\circ \text{C}\) to the vapor phase at \(78 \, ^\circ \text{C}\).
- Express your answer in kilojoules to three significant figures.
\[
Q = \underline{\hspace{3cm}} \, \text{kJ}
\]
Note: This calculation involves multiple steps including heating the ethanol, phase changes, and using specific heat capacities.
Expert Solution
Step 1
For the first part, we have to calculate the heat required to convert 46.0 g of ethanol at -152 oC to the vapor phase at 78 oC.
For the second part, we have to calculate the heat required to convert 46.0 g of ethanol at 34 oC to the vapor phase 78 oC.
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