Chapter 12, Problem 12.133QP

Interpretation Introduction

Interpretation:

• The energy required to warm $2.84\text{ L}$ of water from ${10}^{°}{\text{C to 37}}^{°}\text{C}$ has to be calculated.
• The same amount of water is consumed as ice and the energy required to warm it has to be determined.

Concept Introduction:

Specific heat of a substance refers to the quantity of heat per unit mass of substance that rises the temperature of the substance by one degree Celsius.  The quantity of heat added and the specific heat is related as follows –

$\begin{array}{l}\text{q = m}\times \text{s}\times \Delta \text{T}\\ \text{where q = heat added}\\ \text{ m = mass of the substance}\\ \text{ s = specific heat of the substance}\\ \Delta \text{T = change in Temperature}\\ \end{array}$

Molar heat of vaporization is the heat energy required to boil one mole of a substance at its boiling point.

Molar heat of fusion is the heat energy required to melt one mole of the substance at its melting point.