Advanced Chem Thermodynamics
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Transcript of Advanced Chem Thermodynamics
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// Quiz Feedback | Coursera
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HelpFeedback Thermodynamics
You submitted this quiz on Thu 6 Feb 2014 8:16 AM PST. You got a score of 14.00
out of 14.00.
Question 1
What is the enthalpy of reaction?
C H OH(l) + 3O (g) 2CO (g) + 3H O(l)
H (C H OH(l)) -228 kJ/mol
H (CO (g)) -394 kJ/mol
H (H O(l)) -286 kJ/mol
Your Answer Score Explanation
158 kJ
-908 kJ
-452 kJ
-1418 kJ 1.00
Total 1.00 / 1.00
Question 2
Which process will result in a decrease in the entropy?
Your Answer Score Explanation
N O (g) 2NO (g)
H O(s) H O(l)
2 5 2 2 2
f 2 5
f 2
f 2
2 4 2
2 2
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H O(s) H O(l)
NaCl(s) NaCl(aq)
CO (g) CO (s) 1.00
Total 1.00 / 1.00
Question 3
Which process will be spontaneous?
Your Answer Score Explanation
Sublimation of CO (s) at 1 atm and 25 1.00
Ice melting at -10
NaCl precipitating out of an unsaturated solution
2Fe O (s) 4Fe(s) + 3O (g)
Total 1.00 / 1.00
Question 4
What is S given S = 392 J/K and S = -184 J/K?
Your Answer Score Explanation
-208 J/K
208 J/K 1.00
-576 J/K
576 J/K
Total 1.00 / 1.00
2 2
2 2
2
2 3 2
univ sys surr
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Question 5
What is S at 35C when H = 36 kJ/mol?
Your Answer Score Explanation
117 J/molK
1029 J/molK
-117 J/molK 1.00
-1029 J/molK
Total 1.00 / 1.00
Question 6
When H and S are both positive, what can be said about the spontaneity of the reaction?
Your Answer Score Explanation
Spontaneous at high temperatures because G is
negative.
1.00
Spontaneous at high temperatures because G is
positive.
Spontaneous at low temperatures because G is
negative.
Spontaneous at low temperatures because G is positive.
Total 1.00 /
1.00
surr sys
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Question 7
Find G at 20C when H = 184 kJ and S = 432 J/K.
Your Answer Score Explanation
109 kJ
74.7 kJ 1.00
57.4 kJ
175 kJ
Total 1.00 / 1.00
Question 8
Predict which of the following substances will have the greatest molar entropy?
Your Answer Score Explanation
Ar (g)
B (s)
Cl (g) 1.00
CHCl (l)
Total 1.00 / 1.00
Question 9
Calculate the standard entropy change (S) for the reaction from the given standard entropies
provided in the table.
sys
12
2
3
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C H (g) + 5 O (g) 3 CO (g) + 4 H O(g)
bgcolor="#ff6600">
Substance S(J/mol K)
C H (g) 270.3
O (g) 205.2
CO (g) 213.8
H O(g) 188.8
Your Answer Score Explanation
2155.3 J/K
100.3 J/K 1.00
-72.9 J/K
337.6 J/K
Total 1.00 / 1.00
Question 10
Which of the following is a chemical equation for the free energy for the formation of water?
Your Answer Score Explanation
2 H O(l) 2 H (g) + O (g)
H (g) + O (g) H O(l) 1.00
H (g) + O(g) H O(l)
2 H (g) + O (g) 2 H O(l)
Total 1.00 / 1.00
3 8 2 2 2
.
3 8
2
2
2
2 2 2
2 2 2
2 2
2 2 2
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Question 11
Determine the standard free energy of formation (G ) for C H , given the following information.
All values were measured at 25 C.
C H (g) + 5 O (g) 3 CO (g) + 4 H O(g) G = -2074.2 kJ
bgcolor="#ff6600">
Substance G (kJ/mol)
CO (g) -394.4
H O(g) -228.6
Your Answer Score Explanation
-23.4 kJ/mol 1.00
-1451.2 kJ/mol
-2074.2 kJ/mol
117.0 kJ/mol
Total 1.00 / 1.00
Question 12
The following reaction is allowed to proceed and equilibrium is established. Which statement is
false?
C H (g) + 5 O (g) 3 CO (g) + 4 H O(g) G = -2074.2 kJ
Your Answer Score Explanation
When equilibrium is established, G = 0.0 kJ 1.00
f 3 8
3 8 2 2 2
f
2
2
3 8 2 2 2
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If the reaction initially has one mole of each gas present in
the reaction chamber, the reaction will proceed toward
products to reach equilibrium.
When equilibrium is established, the partial pressures of
CO and H O will both be greater than the partial pressures of
C H and O .
When equilibrium is established, G = 0.0 kJ
Total 1.00 /
1.00
Question 13
Determine G at 25C for the following reaction based on the pressures given in the table.
C H (g) + 5 O (g) 3 CO (g) + 4 H O(g) G = -2074.2 kJ
bgcolor="#ff6600">
Substance P (atm)
C H (g) 10.0
O (g) 13.3
CO (g) 0.0100
H O(g) 0.0500
Your Answer Score Explanation
-2175.7 kJ 1.00
8.921 10 kJ
74.5 kJ
-2074.2 kJ
2 2
3 8 2
3 8 2 2 2
3 8
2
2
2
4
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Total 1.00 / 1.00
Question 14
Determine K for the following reaction at 25C.
H (aq) + F (aq) HF(aq) G = -19.7 kJ
Your Answer Score Explanation
1.3 10
6.8 10
2.8 10 1.00
1.1
Total 1.00 / 1.00
c
+ -
41
-5
3