Chapter 6, Problem 6.48P

(a)

Interpretation Introduction

Interpretation:

The heat flow from $\text{Fe}$ to $\text{Cu}$ or from $\text{Cu}$ to $\text{Fe}$ is to be determined.

Concept introduction:

Heat $\left(q\right)$ is the energy transferred as a consequence of the difference of the temperature between the system and surrounding.

A calorimeter is a device that is employed to measure the heat absorbed or released by the system. A calorimeter is of two types:

1. Coffee cup calorimeter

2. Bomb calorimeter

A bomb calorimeter is employed to determine the heat absorbed or released by the substance placed in the calorimeter at constant volume. A bomb calorimeter is generally used in case of combustion reactions. The heat lost by the reaction is gained by the calorimeter.

$-q_{\text{rxn}}=q_{\text{calorimeter}}$

Coffee cup calorimeter is employed to determine the heat absorbed or released by the substance placed in it at constant pressure. Coffee cup calorimeter is generally used in case of solid that does not dissolve in water. The heat released by the solid is gained by the water and calorimeter.

$-q_{\text{solid}}=q_{\text{water}}+q_{\text{calorimeter}}$

(b)

Interpretation Introduction

Interpretation:

The information that is needed to correct any measurements in an actual experiment is to be determined.

Concept introduction:

Specific heat capacity $\left(c\right)$ of a substance is the amount of heat needed to raise the temperature of $1\text{g}$ of a substance by $1\text{K}$. The formula to calculate heat required is as follows:

$q=\left(\text{mass}\right)\left(c\right)\left(\Delta T\right)$ . (1)

Here,

$\Delta T$ is the temperature difference.

$q$ is the heat released or absorbed.

$c$ is the specific heat capacity of the substance.

The formula to calculate heat required in case of calorimeter is as follows:

$q_{\text{calorimeter}}=\left(C_{\text{calorimeter}}\right)\left(\Delta T_{\text{calorimeter}}\right)$ (2)

Here,

$\Delta T_{\text{calorimeter}}$ is the temperature difference.

$q_{\text{calorimeter}}$ is the heat released or absorbed by calorimeter.

$C_{\text{calorimeter}}$ is the specific heat capacity of the calorimeter.

At the constant volume, the value of heat $\left(q_{\text{v}}\right)$ is equal to internal energy $\left(\Delta E\right)$.

The formula to calculate $\Delta T$ of the system is as follows:

$\Delta T=T_{\text{Final}}-T_{\text{Initial}}$ (3)

(c)

Interpretation Introduction

Interpretation:

The maximum final temperature of the system is to be determined.

Concept introduction:

Specific heat capacity $\left(c\right)$ of a substance is the amount of heat needed to raise the temperature of $1\text{g}$ of a substance by $1\text{K}$. The formula to calculate heat required is as follows:

$q=\left(\text{mass}\right)\left(c\right)\left(\Delta T\right)$ . (1)

Here,

$\Delta T$ is the temperature difference.

$q$ is the heat released or absorbed.

$c$ is the specific heat capacity of the substance.

The formula to calculate heat required in case of calorimeter is as follows:

$q_{\text{calorimeter}}=\left(C_{\text{calorimeter}}\right)\left(\Delta T_{\text{calorimeter}}\right)$ (2)

Here,

$\Delta T_{\text{calorimeter}}$ is the temperature difference.

$q_{\text{calorimeter}}$ is the heat released or absorbed by calorimeter.

$C_{\text{calorimeter}}$ is the specific heat capacity of the calorimeter.

At the constant volume, the value of heat $\left(q_{\text{v}}\right)$ is equal to internal energy $\left(\Delta E\right)$.

The formula to calculate $\Delta T$ of the system is as follows:

$\Delta T=T_{\text{Final}}-T_{\text{Initial}}$ (3)