Consider the chemical reaction,
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$
The rate of this reaction can be expressed in terms of time derivatives of concentration of $N_{2} (g), H_{2} (g) o r N H_{3} (g)$ . Identify the correct relationship amongst the rate expressions.

$R a t e = - \frac{d [N_{2}]}{d t} = - \frac{1}{3} \frac{d [H_{2}]}{d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$

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$R a t e = - \frac{d [N_{2}]}{d t} = - 3 \frac{d [H_{2}]}{d t} = 2 \frac{d [N H_{3}]}{d t}$

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$R a t e = \frac{d [N_{2}]}{d t} = \frac{1}{3} \frac{d [H_{2}]}{d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$

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$R a t e = - \frac{d [N_{2}]}{d t} = - \frac{d [H_{2}]}{d t} = \frac{d [N H_{3}]}{d t}$

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Solution

The correct option is A
$R a t e = - \frac{d [N_{2}]}{d t} = - \frac{1}{3} \frac{d [H_{2}]}{d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$

For any general reaction,
$a A + b B \to c C + d D$
$R a t e = - \frac{1}{a} \frac{d [A]}{d t} = - \frac{1}{b} \frac{d [B]}{d t}$
$= \frac{1}{c} \frac{d [C]}{d t} = \frac{1}{d} \frac{d [D]}{d t}$
$\Rightarrow F o r N_{2} + 3 H_{2} \to 2 N H_{3}$
$R a t e = - \frac{d [N_{2}]}{d t} = - \frac{1}{3} \frac{d [H_{2}]}{d t} = \frac{1}{2} \frac{d [N H_{3}]}{d t}$
$R a t e = k [N_{2} O_{5}]$
$\Rightarrow [N_{2} O_{5}] = \frac{R a t e}{k} = \frac{2.40 \times 10^{- 5}}{3 \times 10^{- 5}} = 0.80 M$

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Similar questions

Consider the chemical reaction

$N_{2} (g) + 3 H_{2} (g) ⟶ 2 N H_{3} (g) .$

The rate of this reaction can be expressed in terms of time derivatives of the concentration of $N_{2} (g), H_{2} (g), o r N H_{3} (g) .$ Identify the correct relationship among the rate expressions.

Q. For the chemical reaction

N_{2}

(g) +

3 H_{2}

(g)

⇌

2 N H_{3}

(g)
The correct option is:

Q. For the reaction;

N_{2} + 3 H_{2} \to 2 N H_{3}

, how does the rate expressions of th reaction inter-relate

\frac{d [H_{2}]}{d t}

and

\frac{d [N H_{3}]}{d t}

Q. The rate of reaction is expressed as rate

= \frac{1}{2} \frac{d [C]}{d t} = - \frac{1}{3} \frac{d [D]}{d t} = \frac{1}{4} \frac{d [A]}{d t} = - \frac{d [B]}{d t}

. The reaction is

Q. For the reaction

2 N O (g) + 2 H_{2} (g) \to N_{2} (g) + 2 H_{2} O (g)

The rate expression can be written in the following ways

\frac{d [N_{2}]}{d t} = k_{1} [N O] [H_{2}] \frac{d [H_{2} O]}{d t} = k [N O] [H_{2}] - \frac{d [N O]}{d t} = k_{1}^{'} [N O] [H_{2}] - \frac{d [H_{2}]}{d t} = k_{1}^{''} [N O] [H_{2}]

The relationship betyween

k, k_{1}, k_{1}^{'}

and

k_{1}^{''}

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Consider the chemical reaction, N2(g)+3H2(g)→2NH3(g) The rate of this reaction can be expressed in terms of time derivatives of concentration of N2(g),H2(g) or NH3(g). Identify the correct relationship amongst the rate expressions.

The correct option is A Rate=−d[N2]dt=−13d[H2]dt=12d[NH3]dt For any general reaction, aA+bB→cC+dD Rate=−1ad[A]dt=−1bd[B]dt =1cd[C]dt=1dd[D]dt ⇒For N2+3H2→2NH3 Rate=−d[N2]dt=−13d[H2]dt=12d[NH3]dt Rate=k[N2O5] ⇒[N2O5]=Ratek=2.40×10−53×10−5=0.80 M

Consider the chemical reaction,
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$
The rate of this reaction can be expressed in terms of time derivatives of concentration of $N_{2} (g), H_{2} (g) o r N H_{3} (g)$ . Identify the correct relationship amongst the rate expressions.