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 **0.322-g sample of phenanthrene (C₁₄H₁₀)** in a bomb calorimeter containing **1050.0 g water**. The temperature increases from **25.30 °C** to **27.70 °C**. The specific heat capacity of water is **4.184 J g⁻¹ °C⁻¹**.The combustion enthalpy is **–7054 kJ/mol phenanthrene**.\[ C_{14}H_{10}(s) + \frac{33}{2} O_2(g) \longrightarrow 14 CO_2(g) + 5 H_2O(l) \quad \Delta H^0 = -7054 \, \text{kJ/mol} \]**Calculate the heat capacity of the calorimeter.**heat capacity of calorimeter = \_\_\_\_\_\_\_\_\_ J/°C

Qcal + Qrxn + Qsol = 0 Qcal = Ccal (T2 - T1) Qrxn = n Δ r Ho Qsol = m Cp (T2 - T1) Given…

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat 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 0.322-g sample of phenanthrene (C14H10) in a bomb calorim containing 1050. g water. The temperature increases from 25.30 °C to 27.70 °C. The specific heat capacity of water is 4.184 J g-l °C-!. The combustion enthalpy is –7054 kJ/mol phenanthrene. C14H10(s) + 33/2 02(g) –14 CO2(g) + 5 H2O(1) A,H° = -7054 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat 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 0.322-g sample of phenanthrene (C14H10) in a bomb calorim containing 1050. g water. The temperature increases from 25.30 °C to 27.70 °C. The specific heat capacity of water is 4.184 J g-l °C-!. The combustion enthalpy is –7054 kJ/mol phenanthrene. C14H10(s) + 33/2 02(g) –14 CO2(g) + 5 H2O(1) A,H° = -7054 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C

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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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 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C