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The rate of formation of nitric oxide (N...

The rate of formation of nitric oxide (NO) in the following reaction is `3.6xx10^(-3) "mol L"^(-1)s^(-1)` .
`4NH_3(g)+5O_2(g)rarr4NO(g)+6H_2O(g)`
Find the rate of disappearance of oxygen.

Text Solution

AI Generated Solution

To find the rate of disappearance of oxygen (O₂) in the given reaction: \[ 4NH_3(g) + 5O_2(g) \rightarrow 4NO(g) + 6H_2O(g) \] we start with the information provided in the question. The rate of formation of nitric oxide (NO) is given as: \[ \text{Rate of formation of NO} = 3.6 \times 10^{-3} \, \text{mol L}^{-1} \text{s}^{-1} \] ...
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For 4NH_3(g)+5O_2(g) hArr 4NO(g)+6H_2O(g) , write the expression of K_c

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Knowledge Check

  • Following reaction is an example of 4NH_(3)(g)+50_(2)(g)overset(Pt(s)) (rarr) 4NO(g) + 6H_(2) O (g)

    A
    Homogeneous catalysis
    B
    Heterogeneous catalysis
    C
    Enzyme catalysis
    D
    Peptization

  • For the reaction , 2C_(2)H_(6)(g)+7O_(2)(g)rarr4CO_(2)(g)+6H_(2)O(l) , the rate of disappearnce of C_(2)H_(6)(g) :

    A
    equals the rate of disappearance of `O_(2)(g)`.
    B
    is seven times the rate of disappearance of `O_(2)(g)`.
    C
    is twice the rate of appearance of `CO_(2)(g)`.
    D
    is one-third the rate of appearance of `H_(2)O(l)`.

  • If the reaction of 1.0 mol NH_(3)(g) and 1.0 mol O_(2)(g)4NH_(3)(g)+5O_(2)(g)to4NO(g)+6H_(2)O(l) is carried to completion, then

    A
    all the `O_(2)(g)` is produced
    B
    4.0 mol NO (g) is produced
    C
    1.5 mol `H_(2)O`(l) is produced
    D
    all the `NH_(3)(g)` is consumed

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