Question

the enthalpy for boiling water is 40.7 kj/mol. what is the quantity of heat (in kj) required to boil 304.1 g of water?

Answer 1

To find the quantity of heat required to boil 304.1 g of water, you need to calculate the heat required to raise the temperature of the water and the heat required for boiling. The total quantity of heat required is 88.53 kJ.

Step-by-step explanation:

To find the quantity of heat required to boil 304.1 g of water, we need to calculate the amount of heat required to raise the temperature of the water to its boiling point and then add the heat required for boiling.

1. First, calculate the heat required to raise the temperature of the water: Q = m * c * ΔT = 304.1 g * 4.184 J/g °C * (100°C - 25°C) = 304.1 g * 75°C * 4.184 J/g °C = 76146.68 J
2. Next, calculate the heat required for boiling: Q = m * ΔHvap = 304.1 g * 40.7 kJ/mol = 304.1 g * 40.7 J/g = 12379.87 J
3. Finally, sum up the two quantities of heat to get the total heat required: Q total = Q1 + Q2 = 76146.68 J + 12379.87 J = 88526.55 J = 88.53 kJ

Therefore, the quantity of heat required to boil 304.1 g of water is 88.53 kJ.