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CHEM_2011_Test_3_Solutions.pdf

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Department
Chemistry
Course Code
CHEM 2011
Professor
Michael Mozurkewich

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CHEM 2011.03 Test #3 November 28, 2012
Page 1 of 4
NAME: Solutions STUDENT NUMBER:________________
You have 50 minutes to complete this test. Calculators are permitted. Other electronics, such as
cell phones and iPods, are not. Make sure they are turned off and put away.
There are 4 questions. There are 30 total marks.
1.000 atm = 1.013 bar = 1.013×105 Pa 1.000 liter = 1000 cm3 = 1.000×10!3 m3
gas constant = 8.314 J K!1 mol!10.00° C = 273.15 K
1. )H°rxn = 29.29 kJ mol!1 for the reaction
Br2(l) + Cl2(g) W 2BrCl(g).
At 298 K, the equilibrium constant for this reaction is 2.03 bar.
[6] Calculate the equilibrium constant for this reaction at 345 K.
Solution:
This will give K2 > K1, as expected for an endothermic reaction.
K2 = 2.03 e1.611 = 10.2 bar (units are not required)

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Description
CHEM 2011.03 Test #3 November 28, 2012 NAME: Solutions STUDENT NUMBER:________________ You have 50 minutes to complete this test. Calculators are permitted. Other electronics, such as cell phones and iPods, are not. Make sure they are turned off and put away. There are 4 questions. There are 30 total marks. 1.000 atm = 1.013 bar = 1.013×10 Pa 5 1.000 liter = 1000 cm = 1.000×10 m !3 3 gas constant = 8.314 J K mol !1 0.00° C = 273.15 K !1 1. )H° rxn= 29.29 kJ mol for the reaction Br 2l) + Cl 2g) W 2BrCl(g). At 298 K, the equilibrium constant for this reaction is 2.03 bar. [6] Calculate the equilibrium constant for this reaction at 345 K. Solution: This will give K 2 K , 1s expected for an endothermic reaction. K 2 2.03 e 1.61= 10.2 bar (units are not required) Page 1 of 4 CHEM 2011.03 Test #3 November 28, 2012 !1 2. At 25.00° C, the standard Gibbs free energychange is 39.30 kJ mol for the reaction 2H O(l) + 2N (g) + 5O (g) W 4HNO (aq) 2 2 2 3 using ideal gas standard states for the gases, the pure liquid standard state for H O(l),2and a dilute solution standard state for HNO (aq)3 All standard states are at one bar pressure. [5] (a) Calculate the equilibrium constant for this reaction at 25.00° C. Solution: K = 1.300 × 10 mol kg bar 4 !4 !5 (units are not required) eq [3] (b) Calculate the activity of HNO (aq)3in equilibrium with 0.78 bar of N (g) and 2.21 bar of O 2g). Ignore the fact that HNO (aq3 undergoes ionic dissociation. Solution: so a HNO3 = 2.38 × 10 mol kg !1 (units are not required) Page 2 of 4 CHEM 2011.03 Test #3
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