Stearic acid [CH3(CH2)16 CO2 H] is a fatty acid, the part of fat that stores most of the energy.

step 1 Hello students in this question we have to calculate the heat released when steric acid was burn

Stearic acid [CH3(CH2)16 CO2 H] is a fatty acid, the part of...

Stearic acid $\left[\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{CO}_{2} \mathrm{H}\right]$ is a fatty acid, the part of fat that stores most of the energy. $1.0 \mathrm{~g}$ of stearic acid was burned in a bomb calorimeter. The bomb had a heat capacity of 652 $\mathrm{~J} /{ }^{\circ} \mathrm{C} .$ If the temperature of $500 \mathrm{~g}$ water $\left(c=4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}\right)$ rose from $25.0$ to $39.3^{\circ} \mathrm{C}$, how much heat was released when the stearic acid was burned? $\left[\right.$ Given $\left.C_{p}\left(\mathrm{H}_{2} \mathrm{O}\right)=4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}\right]$ (a) $39.21 \mathrm{~kJ}$ (b) $29.91 \mathrm{~kJ}$ (c) $108 \mathrm{~kJ}$ $\begin{array}{llll}\text { (d) } 9.32 \mathrm{~kJ} & \therefore \therefore\end{array}$

Stearic acid $\left[\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{CO}_{2} \mathrm{H}\right]$ is a fatty acid, the part of fat that stores most of the energy. $1.0 \mathrm{~g}$ of stearic acid was burned in a bomb calorimeter. The bomb had a heat capacity of 652 $\mathrm{~J} /{ }^{\circ} \mathrm{C} .$ If the temperature of $500 \mathrm{~g}$ water $\left(c=4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}\right)$ rose from $25.0$ to $39.3^{\circ} \mathrm{C}$, how much heat was released when the stearic acid was burned? $\left[\right.$ Given $\left.C_{p}\left(\mathrm{H}_{2} \mathrm{O}\right)=4.18 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}\right]$
(a) $39.21 \mathrm{~kJ}$
(b) $29.91 \mathrm{~kJ}$
(c) $108 \mathrm{~kJ}$
$\begin{array}{llll}\text { (d) } 9.32 \mathrm{~kJ} & \therefore \therefore\end{array}$

Key Concepts

Calorimetry Calculations

Calorimetry calculations involve determining the total energy change in a system by combining the heat absorbed by various components, such as the water and the calorimeter. This usually includes using formulas like Q = m·c·?T for substances, where m is mass, c is specific heat capacity, and ?T is the temperature change, to quantify the energy involved in chemical reactions.

Specific Heat Capacity

Specific heat capacity is a property of a substance that indicates the amount of heat needed to raise the temperature of one gram of the substance by one degree Celsius. This concept is essential in calorimetry experiments where substances like water are used to absorb the energy from a reaction, allowing the temperature change to be directly related to the amount of energy released or absorbed.

Heat Capacity

Heat capacity is the amount of heat required to raise the temperature of an object by one degree Celsius (or Kelvin). In the context of calorimetry, this includes both the heat capacity of the calorimeter itself and any materials, such as water, that absorb the released or absorbed energy, making it pivotal in calculating the total energy transfer during a reaction.

Bomb Calorimeter

A bomb calorimeter is an instrument used to measure the heat released or absorbed during a chemical reaction, typically combustion. It provides a highly controlled environment where a reaction is conducted at constant volume, allowing for the accurate measurement of the energy change of a reaction through the resultant temperature change of the surrounding medium.

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