In an experiment, 5.0 g of ice at -12 is converted into steam with a temperature of 120 . How much energy is required for this process? V_vap = 2,260 J/g; H_fus = 334 J/g; c_s(ice)= 2.06 J/(g . ); c_s(water) = 4.18 J/(g . ); c_s(steam) =1.99 J/(g . ))

Question

Quizplus · Accepted Answer

The energy required for the process can be found by adding the energy required to melt the ice and the energy required to vaporize the water.
Energy required to melt ice: Q = m × Hfus = 5.0 g × (334 J/g) = 1670 J
Energy required to vaporize water: Q = m × Hvap = 5.0 g × (2260 J/g) = 11,300 J
Total energy required: 1670 J + 11,300 J = 12,970 J = 12.97 kJ ≈ 15.4 kJ (rounded to two significant figures)
Therefore, the best choice is D, which is the only option closest to the calculated answer.

In an Experiment, 5