Find the average rate of formation of O_{2(g) | vedclass

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(A) The rate of reaction is expressed as: $Rate = -\frac{1}{2} \frac{\Delta[NO_2]}{\Delta t} = \frac{1}{2} \frac{\Delta[NO]}{\Delta t} = \frac{\Delta[

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

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(A) The rate of reaction is expressed as: $Rate = -\frac{1}{2} \frac{\Delta[NO_2]}{\Delta t} = \frac{1}{2} \frac{\Delta[NO]}{\Delta t} = \frac{\Delta[O_2]}{\Delta t}$ Given that the rate of disappearance of $NO_2$ is $-\frac{\Delta[NO_2]}{\Delta t} = x \ mol \ dm^{-3} \ s^{-1}$. Substituting this into the rate expression: $\frac{\Delta[O_2]}{\Delta t} = \frac{1}{2} \left( -\frac{\Delta[NO_2]}{\Delta t} ight)$ $\frac{\Delta[O_2]}{\Delta t} = \frac{1}{2} 	imes x = \frac{x}{2} \ mol \ dm^{-3} \ s^{-1}$

Find the average rate of formation of $O_{2(g)}$ in the following reaction:
$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$
Given that $\left[-\frac{\Delta[NO_2]}{\Delta t}\right] = x \ mol \ dm^{-3} \ s^{-1}$

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Find the average rate of formation of $O_{2(g)}$ in the following reaction: $2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$ Given that $\left[-\frac{\Delta[NO_2]}{\Delta t}\right] = x \ mol \ dm^{-3} \ s^{-1}$