For the reaction $3\,{A_{\,(g)\,}}\,\xrightarrow{K}\,{B_{(g)}}\, + \,\,{C_{(g)\,,}}K$ is ${10^{ - 14}}\,L/mol.\min .$ if $(A) = 0.5\,M$ then the value of $ - \frac{{d(A)}}{{dt}}$ (in $M / sec$ ) is.

The rate of a gaseous reaction is given by the expression $K\,[A]\,[B]$. If the volume of the reaction vessel is suddenly reduced to $1/4^{th} $ of the initial volume, the reaction rate relating to original rate will be

Write differential rate expression of following reaction and give its order of reaction :

$2 N _{2} O _{5} \rightarrow 4 NO _{2}( g )+ O _{2}$

$C _{4} H _{9} Cl + OH ^{-} \rightarrow C _{4} H _{9} OH + Cl ^{-}$

For a particular reaction, the rate expression is given as $r = k[A] [B]^{0.5}$. If the volume of vessel is reduced to one-fourth of the initial volume, the rate of reaction would

For the reaction, $2A + B\,\to $ products , when the concentrations of $A$ and $B$ both were doubled, the rate of the reaction increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $2.4 \,mol\,L^{-1}\,s^{-1}.$ When the concentration of $A$ alone is doubled, the rate increased from $0.3\,mol\,L^{-1}\,s^{-1}$ to $0.6\,mol\,L^{-1}\,s^{-1}.$ Which one of the following statements is correct?

Reaction $aA + bB\,\to $ product. The rate of reaction $= k[A]^3\, [B]^0$ if the concentration of $A$ is double and concentration of $B$ is half the rate will be ?