A) \[2\]
B) \[-1\]
C) \[1\]
D) \[-2\]
Correct Answer: D
Solution :
Rate of reaction \[=k{{[concentration\text{ }of\text{ }reactant]}^{n}}\] Rate of reaction \[=k{{[B]}^{n}}\] .....(i) where, n = order of reaction. If concentration of B is doubled the rate of reaction decreases by a factor of 4 \[\frac{rate\,\,of\,\,rection}{4}=k{{[2B]}^{n}}\] ?.(ii) Dividing Eqs. (i) by (ii) \[\Rightarrow \] \[\frac{rate\,of\,reaction}{rate\,of\,reaction}\times 4=\frac{k{{[B]}^{n}}}{k{{[2B]}^{n}}}\] \[\Rightarrow \] \[\frac{4}{1}={{\left( \frac{1}{2} \right)}^{n}}\] \[\therefore \] \[n=-2\]
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