Chapter 3.5, Problem 3.36QAP

Interpretation Introduction

(a)

Interpretation:

The mass of water that absorbs 8250 J of heat to raise its temperature from $18.4\text{C}$ to $92.6\text{C}$ should be calculated.

Concept Introduction:

• Specific heat is the amount of heat in joules required to raise the temperature of 1 gram of a substance by $1\text{C}$ . It is expressed in terms of $\text{J/g}\text{C}$
• The amount of heat absorbed or evolved as the temperature changes from T₁ to T₂ is given as:

  $\begin{array}{l}{\text{Q = mcΔT = mc(T}}_{\text{2}}{\text{-T}}_{\text{1}}\text{) -----(1)}\\ \text{m = mass of the substance}\\ \text{c = specific heat}\end{array}$

Interpretation Introduction

(b)

Interpretation:

The mass of silver that loses 3.22 kJ of heat to lower its temperature from $145\text{C}$ to $24\text{C}$ should be calculated.

Concept Introduction:

• Specific heat is the amount of heat in joules required to raise the temperature of 1 gram of a substance by $1\text{C}$ . It is expressed in terms of $\text{J/g}\text{C}$
• The amount of heat absorbed or evolved as the temperature changes from T₁ to T₂ is given as:

  $\begin{array}{l}{\text{Q = mcΔT = mc(T}}_{\text{2}}{\text{-T}}_{\text{1}}\text{) -----(1)}\\ \text{m = mass of the substance}\\ \text{c = specific heat}\end{array}$