Calculate the amount of heat energy required to convert 35.0 g of ice at -12.5°C to water at 24.0°C. (C_water = 4.184 J/g°C; C_ice = 2.03 J/g°C; molar heat of fusion of ice = 6.01 × 10³ J/mol)

Question

Quizplus · Accepted Answer

First, we need to calculate the energy required to raise the temperature of the ice to 0°C:

q1 = m × Cs × ΔT
q1 = 35.0 g × 2.03 J/g°C × (0°C - (-12.5°C))
q1 = 906.125 J

Next, we need to calculate the energy required to melt the ice at 0°C:

q2 = n × ΔHfus
q2 = (35.0 g ÷ 18.015 g/mol) × 6.01 × 10^3 J/mol
q2 = 1.165 × 10^4 J

Finally, we need to calculate the energy required to raise the temperature of the water to 24°C:

q3 = m × Cs × ΔT
q3 = 35.0 g × 4.184 J/g°C × (24.0°C - 0°C)
q3 = 3514.4 J

The total energy required is the sum of q1, q2, and q3:

qtotal = q1 + q2 + q3
qtotal = 1.165 × 10^4 J + 906.125 J + 3514.4 J
qtotal = 1.614 × 10^4 J ≈ 1.61 × 10^14 J

Therefore, the best choice is E, 1.61 × 10^14 J.

Calculate the Amount of Heat Energy Required to Convert 35