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Answer :
Final answer:
To convert 26.0g of ethanol from 23.0°C to a vapor at 78.3°C, the quantity of heat required is -179 kJ.
Explanation:
To calculate the quantity of heat required to convert 26.0g of ethanol from 23.0°C to a vapor at 78.3°C, we need to consider two steps:
First, we need to calculate the heat required to raise the temperature of ethanol from 23.0°C to its boiling point. We can use the formula:
q = m * c * ΔT,
where q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Second, we need to calculate the heat required for the phase change from liquid to vapor. We can use the formula: q = m * ΔH, where q is the heat, m is the mass, and ΔH is the enthalpy of vaporization.
Using the given specific heat capacity (2.746 J/g·°C), enthalpy of vaporization (39.3 kJ/mol), and molar mass of ethanol (46 g/mol), we can calculate the quantity of heat required, which is -179 kJ.
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