Question

The temperature of a sample of water increases from 20.3°C to 45.7°C as it absorbs 5609 J of heat. What is the mass of the sample?

Answer 1

This should help :)

Example 1: A 36.0 g sample of water is initially at 10.0 °C. How much energy is required to turn it into steam at 200.0 °C? (This example starts with a temperature change, then a phase change followed by another temperature change.)

Solution:

q = (36.0 g) (90.0 °C) (4.184 J g¯1 °C¯1) = 13,556 J = 13.556 kJ q = (40.7 kJ/mol) (36.0 g / 18.0 g/mol) = 81.4 kJ q = (36.0 g) (100.0 °C) (2.02 J g¯1 °C¯1) = 7272 J = 7.272 kJ q = 102 kJ (rounded to the appropriate number of significant figures)