Compounds A and B react according to the following chemical equation.
A(g) + 2B(g) →→ 2C(g)
The concentration of either A or B was changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. The following results were obtained. Choose the correct option for the rate equations for this reaction.
Experiment | Initial concentration of [A]/mol L–1 |
Initial concentration of [B]/moI L–1 |
Initial rate (mol L–1 s–1) |
1. 2. 3. |
0.30 0.30 0.60 |
0.30 0.60 0.30 |
0.10 0.40 0.20 |
HINT: Find out the effect of change in rate by changing concentrations of reactant.
Step 1:
The rate of reaction is the change in concentration of reactant with respect to time.
r=k[A]x[B]γ Rate of exp.1 Rate of exp.2=[0.30]x[0.30]y[0.30]x[0.60]y0.100.40=[0.30]γ[0.60]y14=[12]γ[12]2=[12]γy=2
Step 2:
Rate of exp.1 Rate ofexp.3=[0.30]x[0.30]y[0.60]x[0.30]y0.100.20=[0.300.60]x[0.300.30]y12=[12]x[1]y12=[12]xi.e., x=1∴ Rate =k[A]x[B]y Rate =k[A]1[B]2
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