How much heat is required to raise the temperature of 65.8 grams of water from 31.5ºC to 46.9ºC? (The specific heat for water is 4.18 J/g·ºC)

q = (4.18/g' C) * (65.8g) * 4069'C - 31.5'C=4240

4235.7J or 4.2KJ

Explanation:

The heat required to raise the temperature of water is given by

H = mcθ

Where

H = heat required=?

m = mass of the water body=65.8 grams

c = heat capacity of the water = 4.18 J/g·ºC

θ=temperature change = 46.9°C - 31.5°C = 15.4°C

H = 65.8 * 4.18 * 15.4 = 4235.7J or 4.2KJ