The temperature of 1.00 mL of water is raised by 1.00°C for every 4.184 joules of heat absorbed by the water.How many liters of water can be raised from 21.0°C to 100.0°C by the absorption of 8.88 kcal of heat generated by the combustion of natural gas?
A)0.112 L
B)2.13 L
C)37.2 L
D)168 L

Question

Quizplus · Accepted Answer

The amount of heat required to raise the temperature of 1 mL of water by 1°C is 4.184 joules. To convert 8.88 kcal to joules, we use the conversion factor 1 kcal = 4184 joules. Thus, 8.88 kcal = 8.88 * 4184 joules = 37171.52 joules. The temperature difference is 100.0°C - 21.0°C = 79.0°C. The total heat required to raise the temperature of 1 mL of water by 79°C is 4.184 joules/mL/°C * 79°C = 330.536 joules. Therefore, the amount of water that can be heated is 37171.52 joules / 330.536 joules/mL = 112.4 mL, which is 0.112 L.

The Temperature of 1