The initial rates for gaseous reaction A+3B→AB3 are given beloworder of reaction is

# The initial rates for gaseous reaction order of reaction is

1. A

Zero

2. B

Three

3. C

One

4. D

Two

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### Solution:

With respect to A, no change in the rate if the concentration of A is doubled. So the order of ‘A’ is zero.

With respect to B, change in the rate becomes four times $\left({2}^{2}\right)=\frac{0.008}{0.002}=4$if the concentration of B is doubled.

Hence $\mathrm{r}=\mathrm{K}{\left[\mathrm{A}\right]}^{0}{\left[\mathrm{B}\right]}^{2}$

Therefore, total order of reaction is 0+2=2

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