Consider the reaction,
`2A + B rarr C + D` , If the rate expression is `r = K[A]^2[B]^1` and if volume is reduced to `1/3` , the rate of reaction will increases

Consider the reaction, 2A + B rarr C + D , If the rate expression is r = K[A]^2[B]^1 and if volume is reduced to 1/3 , the rate of reaction will increase by

Consider the reaction 2A+B rarr C+D. If the rate expression is rate= K [A]^2 [B]^1 and if concentration of the reactants are increased by three times, the rate of the reaction will increase by:

For the reaction : A + 2B rarr C + D , the expression of rate of reaction will be :

For the reaction : A + 2B rarr C + D , the expression of rate of reaction will be :

For a reaction A + B rarr C + D , the rate equation is, Rate = K[A]^(3/2)[B]^(1/2) . Give the overall order and molecularity of reaction.

For a reaction : 2A + 2B rarr products, the rate law expression is r = k[A]^(2) [B] . Which of the following is/are correct?

For the reaction A+Brarr product, rate law expression for rate = k [A][B]^2 If the volume of the vessel is reduced to 1/3 of its original volume, then what will be the effect on the rate of reaction?

The reaction : 2A +B rarr C + D has the rate equation as: rate = k [A]^x [B]^y What is the molecularity of the reaction?