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WorksheetsEntropy Quiz
Total questions: 19
Worksheet time: 10mins
What does it mean if a reaction is described as spontaneous?
It requires an external catalyst to occur.
It will not occur without continuous energy input.
It will take place of its own accord.
It only occurs under specific laboratory conditions.
Does a spontaneous reaction take into account the rate of reaction?
Yes, it is dependent on the rate of reaction.
No, it does not take account of rate of reaction.
Yes, but only in non-equilibrium conditions.
No, it only depends on temperature.
What is entropy?
A measure of the dispersal of energy in a system which is greater when the system is more ordered
A measure of the dispersal of energy in a system which is greater when the system is more disordered
A measure of the concentration of energy in a system which is greater when the system is more ordered
A measure of the concentration of energy in a system which is greater when the system is more disordered
What is the unit of standard entropy?
Joules per Kelvin (J/K)
Joules per mole (J/mol)
Joules (J)
Kelvin (K)
What is the unit of standard entropy?
J K^-1 mol^-1
J mol^-1
K mol^-1
J K mol
What is the standard enthalpy change of formation (ΔH°f) for ethene (C2H4) according to the thermodynamic data provided?
0 kJ mol^-1
52 kJ mol^-1
131 kJ mol^-1
219 kJ mol^-1
What is the standard entropy (S°) of hydrogen gas (H2) according to the thermodynamic data provided?
0 J K^-1 mol^-1
6 J K^-1 mol^-1
131 J K^-1 mol^-1
219 J K^-1 mol^-1
What is the free energy change for the reaction at 330 K?
+18202 kJ mol^-1
+33.83 kJ mol^-1
+70.15 kJ mol^-1
-18098 kJ mol^-1
What is the free energy change for the reaction of ethene production at 330 K?
A. +18202 kJ mol^-1
B. +33.83 kJ mol^-1
C. -70.15 kJ mol^-1
D. -1089.8 kJ mol^-1
Why is the correct answer for the calculation of ΔG C and not A?
Because ΔH was not calculated correctly.
Because TΔS was not subtracted from ΔH.
Because the units for ΔS were not converted from J K^-1 mol^-1 to kJ K^-1 mol^-1.
Because the value for ΔS was incorrect.
What is the correct expression for calculating ΔG?
ΔG = ΔH + TΔS
ΔG = ΔH - TΔS
ΔG = TΔS - ΔH
ΔG = ΔS - ΔH/T
What is the reason for the incorrectness of answer D?
Because ΔH was not calculated correctly.
Because TΔS was added to ΔH instead of being subtracted.
Because the units for ΔS were not converted from J K^-1 mol^-1 to kJ K^-1 mol^-1.
Because the sign for ΔS was incorrect in the calculation.
Using the information in the table to answer the question. Which of the following is the correct value for the enthalpy change of solution, ΔH°_sol, of calcium fluoride, CaF2?
A. +531 kJ mol^-1
B. -5275 kJ mol^-1
C. +27 kJ mol^-1
D. -1589 kJ mol^-1
Which of the following is the correct value for the enthalpy change of solution, ΔH°_sol, of calcium fluoride, CaF₂?
+531 kJ mol⁻¹
-5275 kJ mol⁻¹
+27 kJ mol⁻¹
-1589 kJ mol⁻¹
What is the correct equation to calculate the enthalpy change of solution, ΔHₛₒₗ?
ΔHₛₒₗ = (ΣΔHₕᵧᵈ) + ΔHₗₐₜₜ
ΔHₛₒₗ = (ΣΔHₕᵧᵈ) - ΔHₗₐₜₜ
ΔHₛₒₗ = [-ΔHₗₐₜₜ + (ΣΔHₕᵧᵈ)]
ΔHₛₒₗ = [-ΔHₗₐₜₜ - (ΣΔHₕᵧᵈ)]
Why is option A incorrect when calculating the enthalpy change of solution for CaF₂?
The value for ΔHₕᵧᵈ F⁻ has been multiplied by 3 instead of 2.
The value for ΔHₕᵧᵈ F⁻ has not been multiplied by 2.
The value for ΔHₕᵧᵈ F⁻ has been multiplied by 2, but ΔHₗₐₜₜ has not been subtracted.
The value for ΔHₕᵧᵈ F⁻ has been multiplied by 2, and ΔHₗₐₜₜ has been added instead of subtracted.
What is the reason for option D being incorrect in the calculation of ΔHₛₒₗ for CaF₂?
The value for ΔHₕᵧᵈ Ca²⁺ and ΔHₕᵧᵈ F⁻ have both been multiplied by 2.
The value for ΔHₕᵧᵈ Ca²⁺ has been multiplied by 2, but ΔHₕᵧᵈ F⁻ has not been multiplied at all.
The value for ΔHₕᵧᵈ Ca²⁺ has not been multiplied by 2, and ΔHₕᵧᵈ F⁻ has been multiplied by 3.
The value for ΔHₕᵧᵈ Ca²⁺ has been multiplied by 3, and ΔHₕᵧᵈ F⁻ has been multiplied by 2.
Wie beeinflusst die Temperatur die Entropie?
Höhere Temperatur führt zu weniger Bewegung der Teilchen und geringerer Entropie.
Bei niedrigerer Temperatur bewegen sich die Teilchen mehr und die Entropie nimmt zu.
Höhere Temperatur verursacht eine geordnetere Anordnung der Teilchen und verringert die Entropie.
Höhere Temperatur führt dazu, dass Teilchen mehr Energie haben und sich mehr bewegen, was zu einer zufälligeren Anordnung und höherer Entropie führt.
Which of the following conditions will mean a reaction is never feasible?
ΔH: Negative, ΔS: Positive, Temperature: High
ΔH: Positive, ΔS: Negative, Temperature: High
ΔH: Negative, ΔS: Negative, Temperature: Low
ΔH: Positive, ΔS: Positive, Temperature: High
