Question

Consider a sample of 11.2 g of ice initially at 0.0 C. How much energy in kilojoules is required to melt the ice and warm it to 22.0 C?

The molecular weight of water is 18.015 g/mol.

PLEASE HELP lol

Answer 1

1034.88J

Step-by-step explanation:

Given that:

mass (m) = 11.2 g, initial temperature = 0°C, final temperature = 22°C, the specific heat capacity of water (C) = 4.2 J/g°C

Temperature difference (ΔT) = final temperature - initial temperature = 22 - 0 = 22°C

The quantity of heat (Q) required to melt the ice can be calculated from the equation:

Q = mCΔT

Q = 11.2 g × 4.2 J/g°C × 22°C

Q = 1034.88J