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The decompoistion of N(2)O(5) according ...

The decompoistion of `N_(2)O_(5)` according to the equation `2N_(2)O_(5)(g) rarr 4NO_(2)(g)+O_(2)(g)`
is a first order reaction. After `30 min`, form the start of the decompoistion in a closed vessel, the total pressure developed is found t be `284.5 mm Hg`. On complete decompoistion, the total pressure is `584.5 mm Hg`. Calculate the rate constant of the reaction.

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The correct Answer is:
`5.2xx10^(-3)min^(-1)`
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The decomposition of N_(2)O_(5) according to the equation: 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) is a first order reaction. After 30 min. from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 min of Hg and on complete decomposition, the total pressure is 584.5 min of Hg. Calculate the rate constant for the reaction.

The decompasition N_(2)O_(5) acccording to the equation. N_(2)O_(5)rarr4NO_(2)(g)+O_(2)(g) is a first order reaction. After 30 minutes from the start of the decomposition is a closed vessel, the total pressure developed is found to be 284. 5 mm Hg and on completion the total pressure is 284.5mm Hg. Calculate the rate constant of the reaction

For the first order reaction 2N_(2)O_(5)(g) rarr 4NO_(2)(g) + O_(2)(g)

For a reaction, 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) rate of reaction is:

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