Question

What quantity of heat (in kJ) would be required to convert 15.1 g of ice to water at 0.00 °C? (∆Hfus = 6.01 kJ/mol for water)

Answer 1

The quantity of heat required to convert 15.1 g of ice to water at 0.00 °C is 5.03 kJ.

Step-by-step explanation:

To calculate the quantity of heat required to convert 15.1 g of ice to water at 0.00 °C, we need to use the formula Q = m * ΔHfus, where Q is the heat required, m is the mass of the ice, and ΔHfus is the heat of fusion for water.

First, convert the mass of ice to moles by dividing by the molar mass of water (18.015 g/mol). Then, multiply the moles of ice by the heat of fusion (6.01 kJ/mol) to find the quantity of heat required.

Since the molar mass of water is 18.015 g/mol, the number of moles of ice is 15.1 g / 18.015 g/mol = 0.838 mol. Therefore, the quantity of heat required is 0.838 mol * 6.01 kJ/mol = 5.03 kJ.