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 content of 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 0.348-g sample of decanoic acid (C10H2002) in a bomb calorimeter containing 1000. g of water. The temperature increases from 26.00 °C to 28.40 °C. The heat capacity of water is 4.184 Jg-l°c-1. The molar heat of combustion is -6080. kJ per mole of decanoic acid. C10H2002(s) + 14 O2(g) 10 CO2(g) + 10 H20(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter J/°C
1. A certain two-step process involves transfer of heat and work between the system and the surroundings. In the first step, the internal energy, AE, of the system increases by 115.4 J when 95.1 J of work is done on the system. In the second step, the internal energy of the system decreases by 32.2 J when 15.6 J of work is done on the surroundings. In the first step of the two-step process, how much heat, in Joules, was absorbed or released? b. How much heat, in Joules, was absorbed or released in the whole two-step process? a.
When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass = 126.75 g/mol) and 6.8 kJ of heat is produced. What is the enthalpy change for the reaction when 1 mole of iron(II) chloride is produced? round to sig figs
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(b) In one experiment, a 25 g sample of an alloy was heated to a certain temperature. The heated alloy was then dropped into a beaker containing 90 g of water at 25.32 °C. The temperature of the water rose to a final value of 27.18 °C. Predict the final temperature that the alloy is being heated at the beginning of the experiment. Given that the heat capacity of water and alloy are 4.184 JgC and 0.3847 Jg l°C-' respectively.
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When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
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