Question

At a pressure of 1 atm, what is H in kJ for the process of condensing a 41.1 g sample of gaseous mercury at its normal boiling point of 357 °C?

A) 41.1 kJ
B) 23.9 kJ
C) 59.3 kJ
D) 357 kJ

Answer 1

To determine the heat (H) in kJ for the process of condensing a 41.1 g sample of gaseous mercury at its normal boiling point of 357 °C, we can use the concept of heat of vaporization.

Step-by-step explanation:

To determine the heat (H) in kJ for the process of condensing a 41.1 g sample of gaseous mercury at its normal boiling point of 357 °C, we can use the concept of heat of vaporization. The heat of vaporization is the amount of heat energy required to change 1 mole of a substance from its liquid state to its gaseous state at a constant temperature and pressure.

Given that the heat of vaporization for mercury is not provided in the question, we can refer to the heat of vaporization for water as a reference point. We know that when 1 mol of water vapor at 100°C condenses to liquid water at 100°C, 40.7 kJ of heat is released into the surroundings. Using this information, we can calculate the heat of vaporization for mercury.

Once we have the heat of vaporization for mercury, we can then multiply it by the number of moles of gaseous mercury to find the heat (H) in kJ for the condensation process.