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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$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.
$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.
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View SolutionWhat is the order and molecularity respectively for the elementary reaction given below?
$O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$
$O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$ if $r = k[O_3][O]$
The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$
Medium
View SolutionFor the reaction $2 NO_{(g)} + 2 H_{2(g)} \longrightarrow N_{2(g)} + 2 H_2O_{(g)}$ with the rate law $\text{rate} = k[NO]^2[H_2]$,what is the order of reaction with respect to $H_2$ and the overall order of reaction,respectively?
The following data are obtained for a reaction,$X + Y \rightarrow$ Products.
$Expt.$ $[X]_0 / mol \ L^{-1}$ $[Y]_0 / mol \ L^{-1}$ $Rate / mol \ L^{-1} s^{-1}$ $1$ $0.25$ $0.25$ $1.0 \times 10^{-6}$ $2$ $0.50$ $0.25$ $4.0 \times 10^{-6}$ $3$ $0.25$ $0.50$ $8.0 \times 10^{-6}$
The overall order of the reaction is:
| $Expt.$ | $[X]_0 / mol \ L^{-1}$ | $[Y]_0 / mol \ L^{-1}$ | $Rate / mol \ L^{-1} s^{-1}$ |
| $1$ | $0.25$ | $0.25$ | $1.0 \times 10^{-6}$ |
| $2$ | $0.50$ | $0.25$ | $4.0 \times 10^{-6}$ |
| $3$ | $0.25$ | $0.50$ | $8.0 \times 10^{-6}$ |
The overall order of the reaction is:
MediumKVPY 2012
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