Find the average rate of formation of NO_{2_{ | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) The rate of reaction is expressed as: $-\frac{1}{2} \frac{\Delta [N_2O_5]}{\Delta t} = \frac{1}{4} \frac{\Delta [NO_2]}{\Delta t} = \frac{\Delta [

Vedclass · Accepted Answer

$2 x \ mol \ dm^{-3} \ s^{-1}$

Vedclass · Answer

(C) The rate of reaction is expressed as: $-\frac{1}{2} \frac{\Delta [N_2O_5]}{\Delta t} = \frac{1}{4} \frac{\Delta [NO_2]}{\Delta t} = \frac{\Delta [O_2]}{\Delta t}$ Given that $-\frac{\Delta [N_2O_5]}{\Delta t} = x \ mol \ dm^{-3} \ s^{-1}$. Substituting this into the rate expression: $\frac{1}{2} (x) = \frac{1}{4} \frac{\Delta [NO_2]}{\Delta t}$ $\frac{\Delta [NO_2]}{\Delta t} = 4 	imes \frac{x}{2} = 2 x \ mol \ dm^{-3} \ s^{-1}$ Therefore,the average rate of formation of $NO_{2_{(g)}}$ is $2 x \ mol \ dm^{-3} \ s^{-1}$.

Find the average rate of formation of $NO_{2_{(g)}}$ in the following reaction:
$2 N_2O_{5_{(g)}} \rightarrow 4 NO_{2_{(g)}} + O_{2_{(g)}}$
Given that $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$

Similar Questions

Explain the relation between the rate of reaction and the stoichiometric coefficients of a balanced chemical equation with examples.

If the rate of disappearance of $N_2O_5$ in the following reaction is $1.2 \times 10^{-5} \ mol \ L^{-1} \ s^{-1}$,the rate of production of $NO_2$ in $mol \ L^{-1} \ s^{-1}$ is:
$2N_2O_{5(g)} \longrightarrow 4NO_{2(g)} + O_{2(g)}$

For the elementary reaction $2 SO_{2(g)} + O_{2(g)} \rightarrow 2 SO_{3(g)}$,identify the correct relation among the following.

Why is the rate of reaction expressed as negative with respect to a reactant? Is the rate of reaction really negative?

The rate of reaction is expressed as
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Find the average rate of formation of $NO_{2_{(g)}}$ in the following reaction: $2 N_2O_{5_{(g)}} \rightarrow 4 NO_{2_{(g)}} + O_{2_{(g)}}$ Given that $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$