Under constant-volume conditions, the heat of combustion of benzoic acid (C₆H₅COOH) is 26.38 kJ/g. A 2.760-g sample of benzoic acid is burned in a bomb calorimeter. The temperature of the calorimeter increases from 21.60 to 29.93 °C. c. Suppose that in changing samples, a portion of the water in the calorimeter were lost. In what way, if any, would this change the heat capacity of the calorimeter?

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Understand that the heat capacity of the calorimeter is the amount of heat required to raise the temperature of the entire calorimeter system by 1 degree Celsius.

Recognize that the calorimeter system includes both the calorimeter itself and the water it contains.

Consider that if water is lost from the calorimeter, the total mass of the system decreases.

Recall that heat capacity is an extensive property, meaning it depends on the amount of substance present.

Conclude that losing water would decrease the heat capacity of the calorimeter, as there is less mass to absorb the heat.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Heat Capacity

Heat capacity is the amount of heat required to change the temperature of a substance by one degree Celsius. In calorimetry, it is crucial for determining how much heat is absorbed or released during a chemical reaction. The heat capacity of a calorimeter is influenced by its mass and the specific heat of the materials it contains, which means any loss of water would alter its overall heat capacity.

Bomb Calorimeter

A bomb calorimeter is a device used to measure the heat of combustion of a substance under constant volume conditions. It consists of a sealed container (the bomb) where the reaction occurs, surrounded by a known quantity of water. The temperature change of the water is used to calculate the heat released by the combustion, making it essential to understand how changes in the system, like water loss, affect the results.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. Different substances have different specific heat capacities, which affects how they absorb and transfer heat. In the context of a calorimeter, if water is lost, the specific heat capacity of the remaining system changes, potentially leading to inaccurate measurements of heat transfer during the combustion process.

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Heat Capacity

Related Practice

Textbook Question

A 2.200-g sample of quinone (C₆H₄O₂) is burned in a bomb calorimeter whose total heat capacity is 7.854 kJ/°C. The temperature of the calorimeter increases from 23.44 to 30.57 °C. b. What is the heat of combustion per mole of quinone?

Textbook Question

A 1.800-g sample of phenol (C₆H₅OH) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/°C. The temperature of the calorimeter plus contents increased from 21.36 to 26.37 °C. a. Write a balanced chemical equation for the bomb calorimeter reaction.

Textbook Question

A 1.800-g sample of phenol (C6H5OH) was burned in a bomb calorimeter whose total heat capacity is 11.66 kJ/°C. The temperature of the calorimeter plus contents increased from 21.36 to 26.37 °C. b. What is the heat of combustion per gram of phenol?

Textbook Question

Consider the following hypothetical reactions: A → B ΔH = +30 kJ B → C ΔH = +60 kJ (b) Construct an enthalpy diagram for substances A, B, and C, and show how Hess's law applies.

Textbook Question

Calculate the enthalpy change for the reaction P₄O₆(s) + 2 O₂(g) → P₄O₁₀(s) given the following enthalpies of reaction: P₄(s) + 3 O₂(g) → P₄O₆(s) ΔH = -1640.1 kJ P₄(s) + 5 O₂(g) → P₄O₁₀(s) ΔH = -2940.1 kJ

Textbook Question

From the enthalpies of reaction 2 C(s) + O₂(g) → 2 CO(g) ΔH = -221.0 kJ 2 C(s) + O₂(g) + 4 H₂(g) → 2 CH₃OH(g) ΔH = -402.4 kJ Calculate ΔH for the reaction CO(g) + 2 H₂(g) → CH₃OH(g)