Multiple Choice
How do you calculate the heat change when a solute with known mass is dissolved in water, considering its lattice energy and heat of hydration?
8. Thermochemistry
Heat Capacity
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What is the total heat required to convert 1 mole of C2Cl3F3 from liquid at 47.6 °C to gas at 47.6 °C, given the specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J g⁻¹ K⁻¹ and 0.67 J g⁻¹ K⁻¹, respectively, and the heat of vaporization is 27.49 kJ mol⁻¹?
A
27.49 kJ
B
28.40 kJ
C
29.10 kJ
D
26.82 kJ
Verified step by step guidance1
Identify the process involved: The problem involves converting 1 mole of C2Cl3F3 from liquid to gas at a constant temperature of 47.6 °C. This is a phase change process, specifically vaporization.
Understand the concept of heat of vaporization: The heat of vaporization is the amount of energy required to convert a substance from liquid to gas at its boiling point without changing its temperature. For C2Cl3F3, this value is given as 27.49 kJ/mol.
Calculate the total heat required: Since the temperature remains constant during the phase change, the total heat required is simply the heat of vaporization. Therefore, the total heat required to vaporize 1 mole of C2Cl3F3 is 27.49 kJ.
Consider the specific heats: Although specific heats are provided, they are not needed for this calculation because the temperature does not change during the phase transition. Specific heats are relevant when calculating heat for temperature changes, not phase changes.
Conclude the solution: The total heat required to convert 1 mole of C2Cl3F3 from liquid to gas at 47.6 °C is equal to the heat of vaporization, which is 27.49 kJ.
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