0.60 mol of steam condenses at 100°C
You have a statement but no question.
how do you calculate the quantity of heat gained or lost?
To calculate the heat released when 0.60 mol of steam condenses at 100°C, we need to use the formula for heat transfer during a phase change.
The heat released or absorbed during a phase change can be calculated using the equation:
Q = n * ΔH
Where:
Q is the heat released or absorbed (in joules)
n is the number of moles of substance involved
ΔH is the enthalpy of the substance (in joules per mole)
First, we need to find the enthalpy of condensation for water. The enthalpy of condensation is the amount of energy released when 1 mole of a substance changes from its gaseous phase to its liquid phase at a given temperature.
The enthalpy of condensation for steam at 100°C is approximately -40.7 kJ/mol or -40,700 J/mol.
Now, we can calculate the heat released:
Q = n * ΔH
Q = 0.60 mol * (-40,700 J/mol)
Q ≈ -24,420 J (rounded to three significant figures)
Therefore, approximately -24,420 J of heat is released when 0.60 mol of steam condenses at 100°C. Note that the negative sign indicates that heat is being released.