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Calorimetry Knowledge-Based Practice

Chemistry · Thermochemistry & Thermodynamics · Chemistry · Energy & Heat in Chemical Processes

5 Chemistry practice questions on Calorimetry. Questions that assess core concepts and understanding.

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Questions

  1. 1.

    To determine the heat capacity of a calorimeter, a student adds 100.0 g of water at 70.0 °C to the calorimeter containing 100.0 g of water at 20.0 °C, and the mixture reaches a final equilibrium temperature of 42.0 °C. Assuming the specific heat capacity of water is 4.18 J/(g⋅∘C)4.18\text{ J}/(\text{g}\cdot{^\circ\text{C}}) and no heat is lost to the external surroundings, what is the heat capacity of the calorimeter?

    • A) 27.3 J/∘C27.3\text{ J}/^\circ\text{C}
    • B) 89.6 J/∘C89.6\text{ J}/^\circ\text{C}
    • C) 114 J/∘C114\text{ J}/^\circ\text{C}
    • D) 532 J/∘C532\text{ J}/^\circ\text{C}
  2. 2.

    When a 4.00 g sample of solid ammonium nitrate, NH4NO3\text{NH}_4\text{NO}_3 (molar mass = 80.0 g/mol), is dissolved in 96.0 g of water at 25.0 °C in a coffee-cup calorimeter, the temperature of the mixture decreases to 21.5 °C. Assuming the resulting solution has a specific heat capacity of 4.18 J/(g⋅∘C)4.18\text{ J}/(\text{g}\cdot{^\circ\text{C}}) and heat exchange with the calorimeter and surroundings is negligible, what is the enthalpy of solution (ΔHsoln\Delta H_{\text{soln}}) of ammonium nitrate in kJ/mol?

    • A) −29.3 kJ/mol-29.3\text{ kJ/mol}
    • B) +29.3 kJ/mol+29.3\text{ kJ/mol}
    • C) +28.1 kJ/mol+28.1\text{ kJ/mol}
    • D) +1.46 kJ/mol+1.46\text{ kJ/mol}
  3. 3.

    When 100.0 mL of 0.500 M HCl and 100.0 mL of 0.500 M NaOH, both initially at 22.0 °C, are mixed in a coffee-cup calorimeter, the temperature rises to 25.4 °C. Assuming the resulting solution has a mass of 200.0 g, a specific heat capacity of 4.18 J/(g·°C), and negligible heat loss to the calorimeter and surroundings, what is the enthalpy of neutralization per mole of H2O formed?

    • A) +56.8 kJ/mol
    • B) -56.8 kJ/mol
    • C) -28.4 kJ/mol
    • D) -2.84 kJ/mol
  4. 4.

    A 0.500 g sample of a fuel is completely burned in a bomb calorimeter that has a heat capacity of 4.50 kJ/°C. If the temperature of the calorimeter increases by 2.40 °C, what is the heat of combustion of the fuel per gram?

    • A) 21.6 kJ/g
    • B) 10.8 kJ/g
    • C) 5.40 kJ/g
    • D) 43.2 kJ/g
  5. 5.

    A 50.0 g sample of an unknown metal heated to 100.0 °C is submerged into an insulated calorimeter containing 100.0 g of water at 22.0 °C. If the final equilibrium temperature of the mixture is 24.0 °C, what is the specific heat capacity of the metal? (Assume no heat loss to the surroundings and that the specific heat capacity of water is 4.18 J/(g⋅∘C)4.18\text{ J}/(\text{g}\cdot{^\circ\text{C}}).)

    • A) 0.84 J/(g⋅∘C)0.84\text{ J}/(\text{g}\cdot{^\circ\text{C}})
    • B) 0.44 J/(g⋅∘C)0.44\text{ J}/(\text{g}\cdot{^\circ\text{C}})
    • C) 0.38 J/(g⋅∘C)0.38\text{ J}/(\text{g}\cdot{^\circ\text{C}})
    • D) 0.22 J/(g⋅∘C)0.22\text{ J}/(\text{g}\cdot{^\circ\text{C}})

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