The rate law equation for a reaction is $R = k[x][y]$. The rate of reaction doubles when:
- Aconcentration of $x$ is kept constant and concentration of $y$ is halved
- Bconcentration of both $x$ and $y$ is doubled
- Cconcentration of $x$ is doubled and concentration of $y$ is kept constant
- Dconcentration of $y$ is doubled and concentration of $x$ is halved
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Similar Questions
Give the relation between half-life $(t_{1/2})$ and initial concentration of reactant $([R]_0)$ for an $(n-1)^{th}$ order reaction.
Which of the following statements regarding the molecularity of a reaction is wrong?
Easy
View SolutionThe initial reaction $2AB + B \to A_2B_3$ is carried out in vessels of volume $1 \ dm^3$ and $2 \ dm^3$ respectively,using equal moles of reactants. The ratio of the reaction rates $(r_1/r_2)$ is:
Medium
View SolutionThe reaction,$X + 2Y + Z \to N$ occurs by the following mechanism:
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?
$(i)$ $X + Y \rightleftharpoons M$ (very rapid equilibrium)
$(ii)$ $M + Z \to P$ (slow)
$(iii)$ $P + Y \to N$ (very fast)
What is the rate law for this reaction?
Medium
View SolutionThe unit of rate constant for a second-order reaction is usually expressed as:
Easy
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