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The initial concentration of N(2)O(5)to ...

The initial concentration of `N_(2)O_(5)to 2NO_(2(g))+(1)/(2)O_(2(g))` was `1.24xx10^(-2)` mol `L^(-1)` at 300 K temperature .The concentration of `N_(2)O_(5)` after 60 minutes was `0.2xx10^(-2)` mol `L^(-1)`.Calculate the rate constatn of the reaction .

Text Solution

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`0.0304 min^(-1)`
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The initial concentration of N_(2)O_(5) in the following first order reaction N_(2)O_(5(g))to2NO_(2(g))+(1)/(2)O_(2(g)) was 1.24xx10^(-2) Mol L^(-1) at 318 K.The concentration of N_(2)O_(5) after 60 minutes was 0.20xx10^(-2) mol L^(-1) . calculate the rate constant of the reaction at 318 K.

Following is first order reaction: N_(2)O_(5) ("solution") to2NO_(2) ("solution")+(1)/(2)_(O_(2)(g)) In which CCl_(4) is a solute .It is k= 5.0xx10^(-4)S^(-1) The concentration of N_(2)O_(5) in initial is 0.25 mol L^(-1) (i)What will be the rate of reaction initially? (ii)Calculate half life (t_(1)/(2)) (iii)How much time require to compute 75 % reaction ? (iv)Calculate the concentration of N_(2)O_(5) and NO after 30 min .

Knowledge Check

  • State the product of reaction : 2SO_(2(g)) + O_(2(g)) + 2H_2 O_((1)) to

    A
    `2H_2 SO_3`
    B
    `2H_2 SO_4`
    C
    `4H_2 SO_4`
    D
    `H_2 SO_4`

  • For the reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)) , the standard equilibrium constant K_P is 5.8xx10^5 at 298 K temperature . If the concentration of gases indicate by mol L^(-1) then find the value of standard equilibrium constant from the following. (R=0.08314 L bar K^(-1) "mol"^(-1) )

    A
    `3.5xx10^6`
    B
    `3.8xx10^7`
    C
    `3.56xx10^(+8)`
    D
    `3.99xx10^9`

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