How much heat, in joules, is required to convert 1.00 kg of ice at 0°C into steam at 100°C? (L_ice = 333 J/g; L_steam = 2.26 × 10³ J/g.)

Question

Quizplus · Accepted Answer

To solve this problem, we need to consider each phase change separately and then add up the energy requirements. The energy required for each phase change is given by the formula:

Energy = mass x (heat of fusion or vaporization)

where mass is the mass of the substance undergoing the phase change, and heat of fusion or vaporization is the energy required to transform one unit of mass of the substance from one phase to another.

First, we need to melt the ice, which requires:

Energy = 1.00 kg x (333 J/g) x (1000 g/kg) = 3.33 x 10^5 J

Next, we need to heat the water from 0°C to 100°C, which requires:

Energy = 1.00 kg x (4.18 J/g°C) x (100°C) = 4.18 x 10^5 J

Finally, we need to vaporize the water into steam, which requires:

Energy = 1.00 kg x (2260 J/g) x (1000 g/kg) = 2.26 x 10^6 J

Adding up these three energy requirements, we get:

Total energy = 3.33 x 10^5 J + 4.18 x 10^5 J + 2.26 x 10^6 J = 3.01 x 10^6 J

Therefore, the best choice is E, 3.01 × 10^16 J.

How Much Heat, in Joules, Is Required to Convert 1