A **bomb calorimeter**, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods.Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as **calibrating** the calorimeter.In the laboratory, a student burns a **0.983-g** sample of **glutaric acid (C₅H₈O₄)** in a bomb calorimeter containing **1170. g** water. The temperature increases from **24.10 °C** to **26.90 °C**. The specific heat capacity of water is **4.184 J g⁻¹ °C⁻¹**.The combustion enthalpy is **–2151 kJ/mol** glutaric acid.\[ \text{C}_5\text{H}_8\text{O}_4(s) + 5 \text{O}_2(g) \longrightarrow 5 \text{CO}_2(g) + 4 \text{H}_2\text{O}(l) \quad \Delta H^\circ = -2151 \text{ kJ/mol} \]**Calculate the heat capacity of the calorimeter.**\[\text{heat capacity of calorimeter} = \boxed{\hspace{20mm}} \, \text{J/°C}\]

Given that: Mass of glutaric acid = 0.983 gMass of water = 1170 gChange in temperature, ∆T = 26.90oC…

In the laboratory a student burns a 0.983-g sample of glutaric acid (C;HgO4) in a bomb calorimete containing 1170. g water. The temperature increases from 24.10 °C to 26.90 °C. The specific heat capacity of water is 4.184 J g-l °C!. The combustion enthalpy is -2151 kJ/mol glutaric acid. C5H2O4(s) + 5 O2(g) 5 CO2(g) + 4 H2O(1) A,H° = -2151 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = | C*/נ

In the laboratory a student burns a 0.983-g sample of glutaric acid (C;HgO4) in a bomb calorimete containing 1170. g water. The temperature increases from 24.10 °C to 26.90 °C. The specific heat capacity of water is 4.184 J g-l °C!. The combustion enthalpy is -2151 kJ/mol glutaric acid. C5H2O4(s) + 5 O2(g) 5 CO2(g) + 4 H2O(1) A,H° = -2151 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = | C*/נ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

A **bomb calorimeter**, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods.

Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as **calibrating** the calorimeter.

In the laboratory, a student burns a **0.983-g** sample of **glutaric acid (C₅H₈O₄)** in a bomb calorimeter containing **1170. g** water. The temperature increases from **24.10 °C** to **26.90 °C**. The specific heat capacity of water is **4.184 J g⁻¹ °C⁻¹**.

The combustion enthalpy is **–2151 kJ/mol** glutaric acid.

\[ \text{C}_5\text{H}_8\text{O}_4(s) + 5 \text{O}_2(g) \longrightarrow 5 \text{CO}_2(g) + 4 \text{H}_2\text{O}(l) \quad \Delta H^\circ = -2151 \text{ kJ/mol} \]

**Calculate the heat capacity of the calorimeter.**

\[
\text{heat capacity of calorimeter} = \boxed{\hspace{20mm}} \, \text{J/°C}
\]

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