Bringing It Together: Question 13.2 A reaction has the stoichiometry: 3A + B C +
ID: 893185 • Letter: B
Question
Bringing It Together: Question 13.2 A reaction has the stoichiometry: 3A + B C + D. The following data were obtained for the initial rate of formation of C at various concentrations of A and B.
Initial Concentration
[A]
[B]
Initial Rate of Formation of C
(mol L-1 s-1)
0.10
0.10
0.040
0.20
0.20
0.16
0.20
0.10
0.16
(a) What is the rate law for the reaction? Rate = k [A]0[B]2 Rate = k [A]2[B]0 Rate = k [A]1[B]1 Rate = k[A]2[B]2 None of these.
(b) What is the rate constant for the reaction? L mol-1 s-1 the tolerance is +/-1 in the 2nd significant digit
(c) What is the rate at which C is formed if [A] = 0.44 M and [B] = 0.75 M? mol L-1 s-1 the tolerance is +/-1 in the 2nd significant digit
Initial Concentration
[A]
[B]
Initial Rate of Formation of C
(mol L-1 s-1)
0.10
0.10
0.040
0.20
0.20
0.16
0.20
0.10
0.16
Explanation / Answer
from Trial 1 and Trial 3
When Concentration of A is doubled without a change in concentration of B, the rate has increased by 4 times. This suggests the rate to be proportional to [A]2 and no dependence of rate on B. This is further confimred that
from Trail 2 , when A is doubled and B is also doubled, there is a four times increase in rate expression
Hence Rate expression reads Rate= K [A]2
Where K is the rate constant
From trial 1
0.040 =K (0.1)2
K =0.040/(0.1)2 = 4 Lmol-1s-1
Rate of formation of C= 4 * [0.44]2 = 0.1936 Mol/L.sec
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