the data for the reaction A + B rightarrow C given in the table 0.250 0.150 0.90

Question

the data for the reaction A + B rightarrow C given in the table 0.250 0.150 0.90 0.250 0.300 35.6 0.500 0.300 712 Determine the order of the reaction for each reactant. calculate the rate constant (k) for the reaction Write the complete rate expression for this reaction. If [A] is 1.0 M and [B]is 0.6M. what is the rate of this reaction? For the second-order reaction below, the initial concentration of reactant A is 0.24 M. If the rate constant for the reaction is 1.5 10^-2 M^-1s^-1. what is the concentration of A after 265 seconds? 2A rightarrow B +C rate = k[A]^2

Explanation / Answer

3)

1)

see experiment 2 and 3:

[A] doubles

[B] is constant

rate doubles

so, oder of A is 1

see experiment 1 and 2:

[A] is constant

[B] doubles

rate becomes 4 times

so, oder of B is 2

overall order = 1 + 2 = 3

2)

rate law can be written as:

rate = k*A*B^2

put values from experiment 1,

8.90 = k*0.25*0.15^2

k = 1582.22 M-2.s-1

3)

rate law can be written as:

rate = k*A*B^2

4)

rate = k*A*B^2

rate =1582.22*1.0*0.6^2

rate = 8.90 M/s

I am allowed to answer only 1 question at a time

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