N O _ 2 required for a reaction is produced by the decomposition of N _ 2 O _ 5 in CC l _ 4 as per the equation, 2 N _ 2 O _ 5 (g) → 4N O _ 2 (g) + O _ 2 (g) . The initial concentration of N _ 2 O _ 5 is 3.00mol L ^ - 1

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Quantrex Academy · Accepted Answer

Correct answer: A. 1.667 × 10 ^ - 2 mol L ^ - 1 ^ - 1

Rate of reaction in terms of rate of disappearance of

{N}_{2}{O}_{5} ( s )

- \dfrac{d\left[{N}_{2}{O}_{5}\right]}{dt} = \dfrac{1}{2}\dfrac{d\left[N{O}_{2}\right]}{dt} = \dfrac{2d\left[{O}_{2}\right]}{dt} = rateofReaction

- \dfrac{( - 3 + 1.75 )}{30} = rateofreaction

- \left(- \dfrac{0.25}{30}\right) = 8.3 \times {10}^{- 3}mol{L}^{- 1}m{in}^{- 1}

= \dfrac{25}{3000} = 8.3 \times {10}^{- 3} = \dfrac{1}{2} \times

rate of formation of

{O}_{2}

8.3 \times {10}^{- 3} = \dfrac{1}{2}\dfrac{d\left[N{O}_{2}\right]}{dt}

1.66 \times {10}^{- 2}m / min = \dfrac{d [ N{O}_{2} ]}{dt}

N O _ 2 required for a reaction is produced by the decomposition of...

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