For the chemical reaction

N_2(g) + 3H_2(g)\leftrightharpoons 2NH_3(g)

the correct option is:

 

  • Option 1)

    -\frac{1}{3}\frac{d[H_2]}{dt} = -\frac{1}{2}\frac{d[NH_3]}{dt}

  • Option 2)

    -\frac{d[N_2]}{dt} = {2}\frac{d[NH_3]}{dt}

  • Option 3)

    -\frac{d[N_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}

  • Option 4)

    {3}\frac{d[H_2]}{dt} ={2}\frac{d[NH_3]}{dt}

Answers (1)
S solutionqc

For a chemical reaction:

aA +bB \longrightarrow cC +dD

The rate is always given as:

-\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B]}{dt} = \frac{1}{c}\frac{d[C]}{dt} = \frac{1}{d}\frac{d[D]}{dt}

\therefore for the reaction:

N_2(g) + 3H_2(g)\leftrightharpoons 2NH_3(g),

Thus, 

-\frac{d[N_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}

Option 3 is correct.


Option 1)

-\frac{1}{3}\frac{d[H_2]}{dt} = -\frac{1}{2}\frac{d[NH_3]}{dt}

Option 2)

-\frac{d[N_2]}{dt} = {2}\frac{d[NH_3]}{dt}

Option 3)

-\frac{d[N_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}

Option 4)

{3}\frac{d[H_2]}{dt} ={2}\frac{d[NH_3]}{dt}

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