Difficult
Write the general equation of a reaction and explain what the order of reaction is. What are its possible values?
(N/A) General Reaction: $aA + bB \rightarrow cC + dD$
The differential rate expression for the reaction is given by:
Rate $= -\frac{d[R]}{dt} = k[A]^x[B]^y$
Here,the values of $x$ and $y$ are determined experimentally and may or may not be equal to the stoichiometric coefficients $a$ and $b$.
The exponents $x$ and $y$ indicate the sensitivity of the reaction rate to changes in the concentrations of $A$ and $B$ respectively.
$(i)$ $x$ represents the order with respect to reactant $A$.
$(ii)$ $y$ represents the order with respect to reactant $B$.
$(iii)$ $(x + y) = \text{Overall order of the reaction}$.
Order of Reaction: The sum of the powers of the concentrations of the reactants in the rate law expression is called the order of that chemical reaction.
The order of a reaction can be $0, 1, 2, 3$ or even a fraction,and these values are always determined experimentally.
The differential rate expression for the reaction is given by:
Rate $= -\frac{d[R]}{dt} = k[A]^x[B]^y$
Here,the values of $x$ and $y$ are determined experimentally and may or may not be equal to the stoichiometric coefficients $a$ and $b$.
The exponents $x$ and $y$ indicate the sensitivity of the reaction rate to changes in the concentrations of $A$ and $B$ respectively.
$(i)$ $x$ represents the order with respect to reactant $A$.
$(ii)$ $y$ represents the order with respect to reactant $B$.
$(iii)$ $(x + y) = \text{Overall order of the reaction}$.
Order of Reaction: The sum of the powers of the concentrations of the reactants in the rate law expression is called the order of that chemical reaction.
The order of a reaction can be $0, 1, 2, 3$ or even a fraction,and these values are always determined experimentally.
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Similar Questions
For the reaction $2A + B \rightarrow C + D$,select the correct rate law based on the following data:
$1$. $[A] = 0.1, [B] = 0.1, \text{Initial Rate} = 7.5 \times 10^{-3}$
$2$. $[A] = 0.3, [B] = 0.2, \text{Initial Rate} = 9.0 \times 10^{-2}$
$3$. $[A] = 0.3, [B] = 0.4, \text{Initial Rate} = 3.6 \times 10^{-1}$
$4$. $[A] = 0.4, [B] = 0.1, \text{Initial Rate} = 3.0 \times 10^{-2}$
$1$. $[A] = 0.1, [B] = 0.1, \text{Initial Rate} = 7.5 \times 10^{-3}$
$2$. $[A] = 0.3, [B] = 0.2, \text{Initial Rate} = 9.0 \times 10^{-2}$
$3$. $[A] = 0.3, [B] = 0.4, \text{Initial Rate} = 3.6 \times 10^{-1}$
$4$. $[A] = 0.4, [B] = 0.1, \text{Initial Rate} = 3.0 \times 10^{-2}$
Easy
View SolutionFor the reaction $A + 2B \to C$,the rate is given by $R = k[A][B]^2$. The order of the reaction is:
For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$ $1$ $0.02$ $0.02$ $2 \times 10^{-2}$ $2$ $0.02$ $0.04$ $4 \times 10^{-2}$ $3$ $0.04$ $0.04$ $8 \times 10^{-2}$
| Entry | $[A]$ in $M$ | $[B]$ in $M$ | Initial rate $(M/s)$ |
|---|---|---|---|
| $1$ | $0.02$ | $0.02$ | $2 \times 10^{-2}$ |
| $2$ | $0.02$ | $0.04$ | $4 \times 10^{-2}$ |
| $3$ | $0.04$ | $0.04$ | $8 \times 10^{-2}$ |
DifficultTS EAMCET 2021
View SolutionThe reaction $2N_2O_5 \rightleftharpoons 4NO_2 + O_2$ follows first order kinetics. Hence,the molecularity of the reaction is
Easy
View SolutionThe reaction rate between two substances $A$ and $B$ is expressed as: $\text{rate} = k[A]^n[B]^m$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the ratio of the new rate to the initial rate will be:
MediumAIEEE 2012
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