Chem+160+Sp+11+Final+Practice - 1 The molar heat of...

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1 1. The molar heat of vaporization of 1-butanol, CH 3 (CH 2 ) 2 CH 2 OH, is 43.82 kJ. This substance boils at 117.8°C at 1 atm. Calculate the boiling point in °C of this substance at 747 mmHg. 2. A new element with molar mass 262 g/mol is found to crystallize with a body- centered unit cell. If its density is 4.62 g/cm 3 , what is its atomic radius? 3. Calculate the Henry’s law constant (in units of mol L –1 atm –1 ) for CO 2 if the solubility of CO 2 (g) in water in a closed container is 3.7 g/L, given that the partial pressure of CO 2 is 2736 mmHg. 4. Commercial nitric acid is 71% by mass HNO 3 . The density of the aqueous solution is 1.42 g/mL. Calculate the molarity of HNO 3 in this solution. 5. What is the normal boiling point of a solution in which benzene is the solvent, given that the freezing point of the solution is 1.00°C? For benzene, K f = 5.12°C/m and K b = 2.53°C/m. The normal boiling point of benzene is 80.10°C, and the normal freezing point of benzene is 5.53°C. 6. What is the osmotic pressure of a solution made from 12.5 g of CaCl 2 in enough water to make 500 mL, if CaCl 2 is 78.5% dissociated at 30°C? 7. When the reaction given below takes place in a 1.0-L flask, 8.0 × 10 4 mol of Br 2 is formed during the first 5.0 sec of the reaction. What is the rate of disappearance of NOBr? 2 NOBr(g) 2 NO(g) + Br 2 (g) 8. For the reaction A + B C + D, determine the rate law from the following data: Experiment [A] 0 [B] 0 Initial rate (M sec 1 ) 1 1.72 M 2.44 M 0.68 2 3.44 M 2.44 M 5.44 3 1.72 M 0.10 M 2.8 x 10 2 9. The rate constant for the second-order decomposition 2A B + C is 0.0012 L/mol sec at a given temperature. Calculate the second half-life for this reaction, given that the initial concentration of A is 0.560 mol/L. 10. For reactions that follow the Arrhenius equation, which of the following will lower the activation energy? X. lower the temperature Y. raise the pressure Z. add a catalyst A. X only E. X and Z B . Y o n l
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2 11. If 2.000 atm of CO is mixed with 0.100 atm of H 2 , what is the partial pressure of H 2 when equilibrium is finally achieved? CO(g) + 3H 2 (g) CH 4 (g) + H 2 O(g) K p = 8.0×10 24 Hint: First react all of the limiting reactant, and then set up an equilibrium table. (Recall homework problem 17.82.) This procedure was also used in problems involving the reaction of weak acid with strong base or of weak base with strong acid. 12.
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This document was uploaded on 10/30/2011 for the course CHEM 160:160 at Rutgers.

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Chem+160+Sp+11+Final+Practice - 1 The molar heat of...

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