Standard Enthalpy of Combustion
Chemistry ⇒ Thermochemistry and Energetics
Standard Enthalpy of Combustion starts at 11 and continues till grade 12.
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Describe how Hess's Law can be used to determine the standard enthalpy of combustion of a substance.
Describe how the enthalpy of combustion of a liquid fuel can be determined experimentally in a school laboratory.
Describe the difference between enthalpy of combustion and enthalpy of formation.
Explain why the enthalpy of combustion of a fuel measured in the laboratory is usually less exothermic than the standard value.
A fuel has a standard enthalpy of combustion of -1500 kJ/mol. If 0.2 mol is burned, what is the energy released?
A hydrocarbon has a standard enthalpy of combustion of -2220 kJ/mol. If 44 g of the hydrocarbon is burned, how much energy is released? (Molar mass = 44 g/mol)
A student burns 0.5 g of ethanol (C2H5OH) and finds that it releases 13.6 kJ of energy. Calculate the enthalpy of combustion per mole of ethanol. (Molar mass of ethanol = 46 g/mol)
Calculate the energy released when 10 g of propane (C3H8) is burned. (Standard enthalpy of combustion of propane = -2220 kJ/mol, molar mass = 44 g/mol)
The standard enthalpy of combustion is always: (1) Positive (2) Negative (3) Zero (4) Variable
Which of the following is a correct definition of standard enthalpy of combustion? (1) The enthalpy change when one mole of a substance is formed from its elements. (2) The enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions. (3) The enthalpy change when one mole of a substance is dissolved in water. (4) The enthalpy change when one mole of a substance is vaporized.
Which of the following is a correct statement about the standard enthalpy of combustion? (1) It is always positive. (2) It is measured at 273 K. (3) It is the enthalpy change for burning one mole of a substance. (4) It is the enthalpy change for burning one mole of oxygen.
Which of the following is a reason why the experimental value of enthalpy of combustion may differ from the standard value? (1) Heat loss to surroundings (2) Incomplete combustion (3) Non-standard conditions (4) All of the above
Fill in the blank: The standard enthalpy of combustion is measured at a pressure of ______ kPa.
Fill in the blank: The standard enthalpy of combustion of a substance is the enthalpy change when ______ mole(s) of the substance is burned.
Fill in the blank: The standard enthalpy of combustion of a substance is usually expressed in units of ______ per mole.
Fill in the blank: The standard enthalpy of combustion of benzene (C6H6) is the enthalpy change for the reaction: C6H6(l) + ______ O2(g) → 6CO2(g) + 3H2O(l)
True or False: The enthalpy of combustion can be measured using a bomb calorimeter.
True or False: The enthalpy of combustion of a substance can be used to calculate its enthalpy of formation using Hess's Law.
True or False: The enthalpy of combustion of graphite is different from that of diamond.
True or False: The standard enthalpy of combustion is an extensive property.
