Entropy
Chemistry ⇒ Thermochemistry and Energetics
Entropy starts at 12 and continues till grade 12.
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See sample questions for grade 12
Describe how entropy changes when a solid is dissolved in a solvent to form a solution.
Describe the relationship between entropy and the number of microstates (W) in a system.
Describe what happens to the entropy of the surroundings when an exothermic reaction occurs at constant temperature and pressure.
Explain the Second Law of Thermodynamics in terms of entropy.
A chemical reaction occurs at 298 K with ΔH = -100 kJ and ΔS = -200 J K-1. Calculate ΔSuniverse.
Calculate the standard entropy change (ΔS°) for the reaction: C(s) + O2(g) → CO2(g), given S°[C(s)] = 6 J K-1 mol-1, S°[O2(g)] = 205 J K-1 mol-1, S°[CO2(g)] = 214 J K-1 mol-1.
Describe how entropy changes when a solid is dissolved in a solvent to form a solution.
Explain why mixing two different gases at constant temperature and pressure increases the entropy of the system.
Which law states that the entropy of a perfect crystal at absolute zero is zero? (1) First Law of Thermodynamics (2) Second Law of Thermodynamics (3) Third Law of Thermodynamics (4) Law of Conservation of Mass
Which of the following best defines entropy? (1) The total energy of a system (2) The measure of disorder or randomness in a system (3) The heat content of a system (4) The amount of work done by a system
Which of the following changes will always result in an increase in entropy? (1) Compression of a gas (2) Freezing of a liquid (3) Vaporization of a liquid (4) Formation of a solid from a solution
Which of the following has the greatest entropy at 298 K? (1) 1 mol of O2(g) (2) 1 mol of O2(l) (3) 1 mol of O2(s) (4) 1 mol of O2(aq)
Fill in the blank: The entropy change for a reversible process is ________.
Fill in the blank: The entropy change for the surroundings when a system absorbs heat at constant temperature is ________.
Fill in the blank: The entropy of a perfectly ordered crystal at 0 K is ________.
The entropy change for the system when 1 mol of ice melts at 0°C (ΔHfus = 6.01 kJ mol-1) is ________ J K-1.
State whether the following statement is true or false: Entropy is a state function.
True or False: Entropy always increases in a spontaneous process in an isolated system.
True or False: Entropy can be negative for a substance at any temperature above absolute zero.
True or False: Entropy is a measure of the energy that is unavailable to do work in a system.
