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The gas phase dicomposition of dinitroge...

The gas phase dicomposition of dinitrogen pentoxide is represented by this equation,
`2N_(2)O_(5)(g)rarr4NO_(2)(g)+O_(2)(g)`
What is the rate of formation of oxygen gas (in mol.`L.s^(-1)`) in an experiment where `0.080` mol of `N_(2)O_(5)` is consumed in a `4.0` L container every `0.20` second?

A

`0.020`

B

`0.050`

C

`0.10`

D

`0.20`

Text Solution

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The correct Answer is:
B
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For the first order reaction 2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g)

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For the reaction, 2N_(2)O_(5) (g) rarr 4NO_(2)(g) + O_(2)(g) , the rate of formation of O_(2) is 0.032 g h^(-1) . (a) Calculate the rate of converison of N_(2)O_(5) in g h^(-1) . (b) Calculate the rate of formation of NO_(2) in g h^(-1) .

The decomposition of N_(2) O_(5) is represented by the equation 2N_(2)O_(5(g)) to 4NO_(2(g)) + O_(2(g)) (a ) How is the rate of formation of NO_(2) related to the rate of formation of O_(2) ? (b ) How is the rate of formation of O_(2) related to the rate of consumption of N_(2)O_(s)?

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