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

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(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 [

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

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(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 $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$

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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 $\left[ -\frac{\Delta [N_2O_5]}{\Delta t} \right] = x \ mol \ dm^{-3} \ s^{-1}$