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(a) Derive the general form of the expre...

(a) Derive the general form of the expression for the half-life of first order reaction.
(b) The decomposition of `NH_(3)` on platinum surface is a zero order reaction. What are the rates of production of `N_(2)" and "H_(2)" if "k=2.5xx10^(-4)" mol"^(-1)" L s"^(-1)` ?

Text Solution

Verified by Experts

`"["(b)(Delta[N_(2)])/(Deltat)=2.5xx10^(-4)"mol L"^(-1)s^(-1),(Delta[H_(2)])/(Deltat)=7.5xx10^(-9)"mol L"^(-1)s^(-1)"]"`
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The decomposition of NH_(3) on platinum surface is zero order reaction. What are the rates of production of N_(2) and H_(2) if k=2.5xx10^(-4)mol^(-1)"L s"^(-1) ?

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Knowledge Check

  • The decomposition of NH_(3) on platinum surface is zero order reaction. What are the rates of production of N_(2) and H_(2) if k=2.5xx10^(-4)mol L^(-1)sec^(-1) ? 2NH_(3)(g)rarrN_(2)(g)+3H_(2)(g)

    A
    `1.25xx10^(-4)Ms^(-1), 3.75xx10^(-4)Ms^(-1)`
    B
    `3.00xx10^(-4)Ms^(-1), 7.50xx10^(-4)Ms^(-1)`
    C
    `2.50xx10^(-4)Ms^(-1), 1.25xx10^(-4)Ms^(-1)`
    D
    `3.75xx10^(-4)Ms^(-1), 2.50xx10^(-4)Ms^(-1)`

  • The decomposition of NH_(3) on platinum surface is zero order reaction the rate of production of H_(2) is (k=2.5xx10^(-4) M s^(-1))

    A
    `2.5xx10^(-4) M s^(-1)`
    B
    `1.25 xx 10^(-4) M s^(-1)`
    C
    `3.75 xx10^(-4) M s^(-1)`
    D
    `5.0 xx10^(-4) M s^(-1)`