What is the reaction A(g) + B(g) + C(g)------------> D(g) Experiment Initial [A] (mol/L) Initial [B]...

What is the reaction A(g) + B(g) + C(g)------------> D(g) Experiment Initial [A] (mol/L) Initial [B] (mol/L) Initial [C] (mol/L) Initial rate (M/s) 1 0.0500 0.0500 0.0100 6.25*^(-3) 2 0.1000 0.0500 0.0100 1.25*^(-2) 3 0.1000 0.1000 0.0100 5*10^(-2) 4 0.0500 0.0500 0.0200 6.25*10^(-3)

1) What is the order with respect to each reactant?

2) Write the rate law

3) Calculate K (using the data from experiment 1)

Solutions

Expert Solution

A               B             C             rate
0.05        0.05        0.01      6.25*10^-3
0.1       0.05         0.01        1.25*10^-2
0.1        0.1          0.01       5*10^-2
0.05   0.05         0.02           6.25*10^-3

a)
consider experiment 1 and 2
Here only the concentraion of A doubles and rate doubles. SO order with respect to A is 1

consider experiment 2 and 3
Here only the concentraion of b doubles and rate becomes 4 times. SO order with respect to B is 2

consider experiment 1 and 4
Here only the concentraion of C doubles and rate remains same. SO order with respect to C is 0

b)
rate law is:
rate = k [A] [B]^2

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

consider experiment 1.
rate = 6.25*10^-3 M/s, [A]= 0.05 M, [B]= 0.05 M

rate = k [A] [B]^2
6.25*10^-3 = k * (0.05)*(0.05)^2
k= 50 M^-2 S-1

queen_honey_blossom answered 10 months ago

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