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Rate of Reaction

How are the r...

Question

How are the rates of the following reaction expressed?
$N_{2 (g)} + 3 H_{2 (g)} \to 2 N H_{3 (g)}$

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Solution

Rate of Reaction = $- \frac{d [N_{2}]}{d t}$ = $- \frac{1}{3} \frac{d [H_{2}]}{d t}$ = $+ \frac{1}{2} \frac{d [N H_{3}]}{d t}$

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Q. 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 and of concentration of

N_{2} (g), H_{2} (g)

N H_{3} (g)

. Identify the correct relationship amongst the rate expressions.

Q. Consider the chemical reaction,

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

.
The rate of reaction can be expressed in terms of time derivative of concentration of

N_{2} (g), H_{2} (g)

N H_{3} (g)

. Identify the correct relationship amongst the rate expressions.

Q. 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 derivative of concentration of

N_{2} (g), H_{2} (g)

N H_{3} (g)

. Identify the correct relationship amongst the rate expressions

Q. Consider the following equilibrium reaction

N_{2} (g) + 3 H_{2} (g) ⇋ 2 {N H}_{3} (g)

. What is the unit of the equilibrium expression for this reaction?

N_{2} (g) + {3 H}_{2} (g) ⇌ 2 {N H}_{3} (g) + h e a t

For the reaction above, what is the equilibrium expression?

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