# A 126010 v m s k b c 084010 v m s k d 042010 v m s k

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a.1.260×10%VM ∙ s%Kb.࠵?. ࠵?࠵?࠵?×࠵?࠵?%࠵?࠵?࠵?%࠵?c.−0.840×10%VM ∙ s%Kd.−0.420×10%VM ∙ s%Ke.0.420×10%VM ∙ s%K
4.For the reaction 2 AB + 3 C, the rate of change of A is−0.420×10%VM ∙ s%K. What is the reaction rate?
5.The reaction A + 3 BProducts has an initial rate of 0.0345 M/s and the rate law rate =k[A]2[B]. What will the initialrate be if [A] isquadrupledand [B] ishalved?
6.Determine the rate law given for the following reaction given the initial rate data in the table:
2 A + 2 BC + 2 DExperiment[A] (M)[B] (M)Initial rate (M/s)10.04220.1132.35×10%p20.08440.1139.40×10%p30.08440.2261.88×10%r
7.Use these data for the reaction A2 B to calculate the average rate of change fromt= 0.0 s tot= 50.0 s.Time (s)0.05.010.015.030.050.0[B] (M)00.0350.0720.0980.1770.241
8.Consider the initial rate data collected at 298 K for the reaction shown below. Determine the missing value in thetable.Hint: first determine the rate law and the rate constant.CH3Br(aq) + OH(aq) → CH3OH(aq) + Br(aq)Experiment[CH3Br] (M)[OH] (M)Initial rate (M/s)10.120.121.3 × 10−520.240.122.6 × 10−530.120.066.7 × 10−640.0950.18?
9.The first-order reaction A → B has a rate constant of 0.0643 s−1. How many seconds will it take for 35.2% of A toreact?
10.For a certain first-order reaction at a certain temperature, it takes 8.5 min for the reactant concentration todecrease from 0.66 M to 0.33 M. How much time will it take for the reactant concentration to decrease from 0.88 Mto 0.22 M at the same temperature?
e.25 min11.The decomposition reaction AB → A + B is a second-order process with a rate constant of 6.92 × 10−3M−1·s−1. Theinitial concentration of A is 0.0248 M. Calculate the concentration of A after 78.9 min.a.0.0137 Mb.73.1 Mc.0.0305 Md.0.0245 Me.40.9 M

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Term
Fall
Professor
Arnulfo Mar
Tags
Rate equation, affecting reaction rate
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