For the reaction below, the following data were obtained at constant temperature

Question

For the reaction below, the following data were obtained at constant temperature. Reaction: A(g) + B(g) + C(g) D(g) Exp't Initial [A] (mol/L) Initial [B] (mol/L) Initial [C] (mol/L) Initial Rate (mol/Ls) 1 0.0100 0.0500 0.0100 1.13 10-3 2 0.0200 0.0500 0.0100 2.25 10-3 3 0.0200 0.1000 0.0100 9.00 10-3 4 0.0100 0.0500 0.0200 1.13 10-3 (a) What is the order with respect to each reactant? Select one:(zero order, or half order or first order or second order or third order) with respect to [A]. Select one:(zero order, or half order or first order or second order or third order) with respect to [B]. Select one:(zero order, or half order or first order or second order or third order) with respect to [C]. (b) Select the rate law. a)rate = k[A][B]2 b)rate = k[A]1/2[B][C]1/2 c)rate = k[A]2[C] d)rate = k[A]3[B]3[C]2 e)rate = k[A][B][C] f)rate = k[B]1/2[C]3 (c) What is the value of k from trial 1? ____________ L2/mol2s

Explanation / Answer

a) since the rate doubles whenreactantA doubles then then reaction is first order with respect to [A]

since the rate goes up 4 fold when reactant b is doubled the reaction is second order with respect to [B]

since the rate remains the same when more of reactant C is added the rate is zero order with respect to [C]

the reaction has an overall rate of order 3

b) rate=k[A][B]^2

c) k=rate/[A][B]^2
=1.8x10^-2/0.01*0.2^2
=45 L^2/mol^2*s

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