SQSM-10 - Chapter 10 Chemical Kinetics 1. Distinguish...

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Chapter 10 Chemical Kinetics 10-1 0 10 20 30 40 50 60 70 80 90 100 110 120 time/seconds 0.003 0.004 0.005 0.006 0.007 0.008 0.009 0.010 [NO ] 2 0.004 M 45 s a b 0.0015 M 50 s 1. Distinguish between kinetic and thermodynamic regions of a reaction. Concentrations change in the kinetic region, but they are constant at their equilibrium values in the thermodynamic region. 3. How does an increase in temperature affect the rate of reaction? Increasing the temperature increases the rate of any reaction. 5. Why do reaction rates slow as the reaction proceeds? As the reaction proceeds, the reactant concentrations drop, which causes the reactions to slow. 7. Distinguish between an average and instantaneous rates of reaction. An average rate is a change in concentration divided by the time required to produce the change. An instantaneous rate is the rate at which the concentration is changing at any given instant. 9. Consider the following plot of [NO 2 ] versus time. a) What is the average rate of disappearance of NO 2 over the time of the experiment? −× -5 -1 2 [NO ] (0.0100 M - 0.0034 M) = = 5.5 10 M s t (0 s - 120 s) To determine the instantaneous rates, determine the slopes of the tangent lines at the two times. The tangent lines are drawn in the above figure b) Use the graphical methods presented in Section 10.1 to determine the rate of disappearance of NO 2 at 20 seconds : -5 -1 2 [NO ] (0.0090 M - 0.0050 M) = = 9 10 M s t (3 s - 48 s) at 80 seconds: -5 -1 2 [NO ] (0.0050 M - 0.0035 M) = = 3 10 M s t (58 s - 108 s) 11. What is the rate of formation (M . s -1 ) of NOBr gas in a reaction in which 13.4 mmol of NOBr is produced in a 38.9 mL flask in 26.8 minutes? ∆× ×⋅ × -6 -7 -1 [NOBr] (13.4 10 mol)/0.0389 L = = 2.14 10 M s 60 s t 26.8 min min 13. What are the rates of appearance of NO 2 and O 2 when the rate of disappearance of N 2 O 5 is 2.0x10 -5 M . s -1 ? 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) Define the rates of appearance of NO 2 and O 2 in terms of the rate of disappearance of N 2 O 5 by using the coefficients from the equation. [ ] [ ] [ ] ∆∆ ×× 22 5 2 -5 -5 -1 NO N O NO 11 4 = = (2.0 10 ) = 4.0 10 M s 4t 2t t 2 [ ] [ ] [ ] 5 2 -5 -5 -1 ON O O = = (2.0 10 ) = 1.0 10 M s t2 t t 2 15. What is an exponential decay? What type of kinetics is characterized by an exponential decay? A function, such as y = e -ax , that decreases exponentially is an exponential decay. First order kinetics are characterized by an exponential decay.
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Chemical Kinetics 10-2 17. A reaction has the experimentally determined rate law: rate = k[A][B] 2 . a) What is the reaction order? In a rate law, the sum of all the exponents in the rate law is called the overall order of the reaction. overall order = 1+2 = 3 b) What is the order with respect to A? The exponent on each reactant exponent is referred to as the reactant order ; in this case the order with respect to reactant A is 1. c) What is the order with respect to B? The concentration of B is squared in the rate law, so the reaction is second order with respect to B.
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This note was uploaded on 01/27/2011 for the course CHEM 201 taught by Professor Wilson during the Spring '10 term at N.C. Central.

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SQSM-10 - Chapter 10 Chemical Kinetics 1. Distinguish...

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