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Decomposition of N(2)O(5) in liquid "C...

Decomposition of `N_(2)O_(5)` in liquid `"CCl"_(4)` is a first order reaction : `2N_(2)O_(5)rarr4NO_(2)+O_(2)` . The rate constant for this reaction is `3.66xx10^(-2) "min"^(-1)`.
Determine the reaction -rate when the concentration of `N_(2)O_(5)=3.15"mol .L"^(-1)`

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Verified by Experts

Decomposition of `N_(2)O_(5)` is a first order reaction.
Hence , reaction -rate `k[N_(2)O_(5)]`
Given , rate constant , `k=3.66xx10^(-2)xx3.66xx10^(-2)"min"^(-1)`
`[N_(2)O_(5)] = 3.15 "mol".L^(-1)`
Reaction -rate = `k[N_(2)O_(5)]=3.66xx10^(-2)xx3.15`
= `0.1153"mol".L^(-1)."min"^(-1)`
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Decomposition of N_(2)O_(5) in liquid "CCl"_(4) is a first order reaction : 2N_(2)O_(5)rarr4NO_(2)+O_(2) . The rate constant for this reaction is 3.66xx10^(-2) "min"^(-1) . At what concentration of N_(2)O_(5) will the reaction -rate be 3.854xx10^(-2)"mol.L"^(-1)."min"^(-1) ?

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  12. For the reaction , 4NH(3)(g)+5O(2)(g)rarr4NO(g)+6H(2)O(g) the concentr...

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