Question

A 73-g ice cube at 0°C is heated until 65.1 g has become water at 100°C and 7.9 g has become steam at 100°C. How much energy was added to accomplish the transformation? Answer is in kJ.

Answer 1

To calculate the energy required to accomplish the transformation, we need to use the formula:

Q = m * ΔH

where Q is the energy required, m is the mass of the substance, and ΔH is the enthalpy of transformation.

First, we need to calculate the energy required to melt the ice cube:

Q1 = 65.1 g * 334 J/g = 21783.4 J

Next, we need to calculate the energy required to vaporize the water:

Q2 = 7.9 g * 2260 J/g = 17894 J

The total energy required is:

Q = Q1 + Q2 = 39677.4 J = 39.6774 kJ

Therefore, the energy required to accomplish the transformation is 39.6774 kJ.