Title: Chapter 5: Thermochemistry
Course: Test

Q: If ΔH = -54.74 kJ for a chemical reaction, that reaction _____________.
- is exothermic
- is endothermic
- cannot occur
A: is exothermic

Q: A _____ is an experimental set-up that can be used to measure the heat of a chemical reaction or a physical change and determine the specific heat capacity of a substance.
- manometer
- thermometer
- calorimeter
A: calorimeter

Q: The following can be used to measure the heat of combustion for an unknown sample?
- bomb manometer
- bomb calorimeter
- coffee-cup calorimeter
A: bomb calorimeter

Q: Coffee-cup calorimetry is carried out at _____.
- constant-volume
- constant-pressure
- constant-mass
A: constant-pressure

Q: Bomb calorimetry is carried out at _____.
- constant-volume
- constant-pressure
- constant-mass
A: constant-volume

Q: You are asked to design an experiment to measure the enthalpy of a given reaction. The reaction needs to be at atmospheric pressure so which of the following techniques would be ideal for this experiment?
- bomb manometry
- bomb calorimetry
- coffee-cup calorimetry
A: coffee-cup calorimetry

Q: Your task is to measure the amount of energy evolved during the combustion of some hydrocarbon. Which of the following would be the ideal technique for this experiment?
- coffee-cup calorimetry
- bomb calorimetry
- bomb manometry
A: bomb calorimetry

Q: 100 mL of a 0.300 M solution of AgNO_3 reacts with 100 mL of a 0.300 M solution of HCl in a coffee-cup calorimeter and the temperature rises from 21.80 °C to 23.20 °C. Assuming the density and specific heat of the resulting solution is 1.00 g/mL and 4.18 J/g ∙ °C, respectfully, what is the ΔH°_rxn?
- -39.0 kJ/mol
- +39.0 kJ/mol
- +1.17 kJ/mol
A: -39.0 kJ/mol

Q: Given the ∆H°_f, calculate the ∆H°_rxn for the formation of diamond from graphite.

∆H°_f (C, graphite) = 0 kJ/mol

∆H°_f (C, diamond) = 2 kJ/mol
- 0 kJ/mol
- +2 kJ/mol
- -2 kJ/mol
A: +2 kJ/mol

Q: Calculate the ∆H°_rxn for the combustion of methane using the given ∆H°_f.

∆H°_f, methane(g) = -74.60 kJ/mol;∆H°_f, water(l) = -285.8 kJ/mol

∆H°_f, carbon dioxide(g) = -393.5 kJ/mol
- -1.04 x 10^+3 kJ/mol
- -890.5 kJ/mol
- 890.5 kJ/mol
A: -890.5 kJ/mol

Q: A drop in water temperature is observed when 0.873 g of ammonium nitrate is added. The enthalpy change for this reaction is +0.280 kJ. Which of the statements is accurate?
- The ∆H°_soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.
- The ∆H°_soln for ammonium nitrate is -25.7 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.
- The ∆H°_soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is released into the surroundings.
A: The ∆H°_soln for ammonium nitrate is +25.7 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.

Q: An increase in water temperature is observed when 1.97 g of NaOH is added. The enthalpy change for this reaction is -2.19 kJ. Which of the statements is accurate?
- The ∆H°_soln for NaOH is +44.5 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.
- The ∆H°_soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.
- The ∆H°_soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is absorbed from the surroundings.
A: The ∆H°_soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.

Q: If ∆H = -73.54 kJ for a chemical reaction, that reaction _____________.
- is exothermic
- is endothermic
- cannot occur
A: is exothermic

Q: A chemical reaction that gives off energy in the form of heat is considered _____.
- exothermic
- endothermic
- exergonic
A: exothermic

Q: A chemical reaction that absorbs energy in the form of heat is considered _____.
- exothermic
- endothermic
- exergonic
A: endothermic

Q: A reaction requires a sample to be heated using a water bath near boiling temperature. Which statement below would be accurate?
- Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires -40.7 kJ of energy.
- Boiling water is an exothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.
- Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.
A: Boiling water is an endothermic process and to break apart the intermolecular forces that hold together the water molecules requires +40.7 kJ of energy.

Q: A reaction where the products are lower in energy than the reactants is an example of an _____.
- endothermic process
- exothermic process
- endergonic process
A: exothermic process

Q: A reaction where the products are higher in energy than the reactants is an example of an _____.
- endothermic process
- exothermic process
- exergonic process
A: endothermic process

Q: An _____ reaction results when the energy required to break bonds in the reactants is greater than the energy released by the formation of products.
- exergonic
- endothermic
- exothermic
A: endothermic

Q: An _____ reaction results when the energy released by the formation of products is greater than the energy required to break the bonds in the reactants.
- exergonic
- endothermic
- exothermic
A: exothermic