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The decompasition N(2)O(5) acccording to...

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 584.5mm Hg. Calculate the rate constant of the reaction

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To solve the problem regarding the decomposition of \( N_2O_5 \) and to calculate the rate constant of the reaction, we will follow these steps: ### Step 1: Write the balanced equation The decomposition of \( N_2O_5 \) is given by: \[ N_2O_5 \rightarrow 4NO_2(g) + O_2(g) \] ...
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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.

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

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