For a reaction \(A \rightarrow2B\) The value of K=\(2.5\times10^{-2}sec^{-1}\) .If the reaction had started with 2M of A what will be initial rate of the reaction?

The specific rate of reaction is 1.5 xx 10^(-4) lit "mole"^(-1)."sec"^(-1) . If the reaction is connected with 0.2 mole/lit of of the reactant, the initial rate of the reaction in mole "lit"^(-1) sec^(-1) is

In the II order reaction: \(2A \rightarrow A_{2}\) .The rate of formation of \(A_{2}\) is \(10^{-5}M sec^{-1}\) at 0.01M concentration of A . Calculate the rate constant in the rate of disappearance of A.

Define elementary reaction. For the reaction,\(A \rightarrow Products\), rate is \(1.25\times10^{-2}M/s\) when [A]=0.45M.Determine the rate constant if the reaction is.second order in A

In the II order reaction 2A rightarrow A _(2) .The rate of formation of A_(2) is 10^(-5) M sec ^(-1) at 0.01M concentration of A . Calculate the rate constant in the rate of disappearance of 'A:

In the II order reaction: 2A rightarrow A_(2) .The rate of formation of A_(2) is 10^(-5) M sec^(-1) at 0.01M concentration of A .Calculate the rate constant and the rate of disappearance of 'A'

For a reaction A \rightarrow B , K is 1xx10^(-2)Lmol^(-1)sec^(-1) .If conc of A is 2.0 molL^(-1) ,the rate of reaction would be

Ethylene is produced as: \(C_{4}H_{8}\rightarrow 2C_{2}H_{4}\).The rate constant is \(2.5\times10^{-5}s^{-1}\) .Order of the reaction is

For the reaction, 2A + B+C rarr A_(2)B+C The rate = k[A][B]^(2) with K = 2.0 xx 10^(-6) M^(-2) s^(-1) . Calculate the initial rate of the reaction when [A] = 0.1M, [B] = 0.2M and [C] = 0.8M . IF the rate of reverse reaction is negligible then calculate the rate of reaction after [A] is reduced to 0.06M .

The specific reaction rate constant for a first order reaction is 1xx10^(-2)s^(-1) . If the initial concentration is 1 M , find the initial rate . What is the reaction rate after two minutes ?