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.

exp't initial A initial B initial C initial rate

1 0.0100 0.02000 0.0200 2.12* 10^-2

2 0.0200 0.02000 0.0200 4.24*10^-2

3 0.0200 0.04000 0.0200 1.70*10^-1

4 0.0100 0.02000 0.0400 2.12*10^-2

(a) What is the order with respect to each reactant

.............order with respect to [A]

.............order with respect to [B]

...............order with respect to[C]

(b)the rate low...........

(c) What is the value of k from trial 1?

For the reaction below, the following data were obtained at constant temperature. Reaction: A(g) + B(g) + C(g) exp't initial A initial B initial C initial rate 1 0.0100 0.02000 0.0200 2.12* 10^-2 2 0.0200 0.02000 0.0200 4.24*10^-2 3 0.0200 0.04000 0.0200 1.70*10^-1 4 0.0100 0.02000 0.0400 2.12*10^-2 (a) What is the order with respect to each reactant .............order with respect to [A] .............order with respect to [B] ...............order with respect to[C] (b)the rate low........... (c) What is the value of k from trial 1?

Explanation / Answer

a,we can calculate order using trial 1 and 2 for a

(0.0100/0.0200)x =(2.12* 10^-2/4.24*10^-2)=0.5 so x =1

the order of the reaction with respect to A is 1.

in the same way the order of the reaction with respect to B is 2.

the order of the reaction with respect to c is 0

b, rate =k[A][B]2

c,k=rate/[A][B]2 =2.12* 10^-2/4x10^-6=5300

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