For each of the following reactions express the given rate of change of concentration of the reactant or product in terms of the rate of change of concentration of other reactants or products in that reaction:
$(a)$ $H_{2} O_{2} + 2 H^{+} + 3 I^{-} ⟶ {I_{3}}^{-} + 2 H_{2} O$ ; $- \frac{d [I^{-}]}{d t} =$ ?; $- \frac{d [H^{+}]}{d t} =$ ?
$(b)$ $16 H^{+} + 2 {M n O_{4}}^{-} + 10 I^{-} ⟶ 2 {M n}^{2 +} + 8 H_{2} O + 5 I_{2}$ ; $- \frac{d [M n {O_{4}}^{-}]}{d t} =$ ?
$(c)$ $4 N H_{3} + 5 O_{2} ⟶ 4 N O_{2} + 6 H_{2} O$ ; $- \frac{d [N H_{3}]}{d t} =$ ?

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Solution

a) $\frac{- 1}{3} \frac{d [I^{-}]}{d t} = \frac{- 1}{2} \frac{d [H^{+}]}{d t} = \frac{d [I_{3}^{-}]}{d t}$

b) $\frac{- 1}{2} \frac{d [{M n O}_{4}^{-}]}{d t} = \frac{- 1}{16} \frac{d [H^{+}]}{d t} = \frac{- 1}{10} \frac{d [I^{-}]}{d t} = \frac{1}{2} \frac{d [{M n}^{2 +}]}{d t} = \frac{1}{5} \frac{d [I_{2}]}{d t}$

c) $\frac{- 1}{4} \times \frac{d [{N H}_{3}]}{d t} = \frac{- 1}{5} \frac{d [O_{2}]}{d t} = \frac{1}{4} \frac{d [{N O}_{2}]}{d t}$

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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.

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.