(A) The rate of reaction is given by:$r = -\frac{d[N_2O_5]}{dt} = \frac{1}{2} \frac{d[NO_2]}{dt} = \frac{1}{1/2} \frac{d[O_2]}{dt}$Substituting the gi

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(A) The rate of reaction is given by:$r = -\frac{d[N_2O_5]}{dt} = \frac{1}{2} \frac{d[NO_2]}{dt} = \frac{1}{1/2} \frac{d[O_2]}{dt}$Substituting the given rate expressions:$K_1[N_2O_5] = \frac{1}{2} K_2[N_2O_5] = 2 K_3[N_2O_5]$Dividing by $[N_2O_5]$:$K_1 = \frac{K_2}{2} = 2K_3$Multiplying by $2$:$2K_1 = K_2 = 4K_3$

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Difficult

For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

A
$2K_1 = K_2 = 4K_3$
B
$K_1 = K_2 = K_3$
C
$2K_1 = 4K_2 = K_3$
D
None of these

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

The alkaline hydrolysis of an ester is a .......

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For a chemical reaction $Y + 2Z \to$ Product,the rate-controlling step is $Y + \frac{1}{2}Z \to Q$. If the concentration of $Z$ is doubled,the rate of reaction will:

Difficult

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For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$
$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$
$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$
The correct relation between $K_1, K_2$ and $K_3$ is:

MediumTS EAMCET 2024

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The half-life periods of decomposition of $PH_3$ for different initial pressures are given below $:$
Initial Pressure $p$ (torr) $707$ $79$ $37.5$
Half-life $t_{1/2}$ (min) $84$ $84$ $84$
Determine the order of the reaction.

Medium

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For the reaction $XA + YB \rightarrow mp + nq$,the rate is given by $\text{Rate} = K[A]^c[B]^d$. What is the overall order of the reaction?

Medium

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Initial Pressure $p$ (torr)	$707$	$79$	$37.5$
Half-life $t_{1/2}$ (min)	$84$	$84$	$84$

For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,$\frac{d[O_2]}{dt} = K_3[N_2O_5]$What is the relationship between $K_1$,$K_2$,and $K_3$?

Similar Questions

The alkaline hydrolysis of an ester is a .......

For a chemical reaction $Y + 2Z \to$ Product,the rate-controlling step is $Y + \frac{1}{2}Z \to Q$. If the concentration of $Z$ is doubled,the rate of reaction will:

For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$The correct relation between $K_1, K_2$ and $K_3$ is:

The half-life periods of decomposition of $PH_3$ for different initial pressures are given below $:$ Initial Pressure $p$ (torr)$707$$79$$37.5$Half-life $t_{1/2}$ (min)$84$$84$$84$ Determine the order of the reaction.

For the reaction $XA + YB \rightarrow mp + nq$,the rate is given by $\text{Rate} = K[A]^c[B]^d$. What is the overall order of the reaction?

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For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?

For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$
$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$
$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$
The correct relation between $K_1, K_2$ and $K_3$ is:

The half-life periods of decomposition of $PH_3$ for different initial pressures are given below $:$
Initial Pressure $p$ (torr) $707$ $79$ $37.5$
Half-life $t_{1/2}$ (min) $84$ $84$ $84$
Determine the order of the reaction.