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Factors Affecting the Rate of a Chemical Reaction

The reaction ...

Question

The reaction $2 H_{2} (g) + 2 N O (g) \to 2 H_{2} O (g) + N_{2} (g)$ is first order in $H_{2}$ and second order in $N O$ . The rate constant of the reaction at a certain temprature is 0.42 $M^{- 2} S^{- 1}$ . Calculate the rate when $[H_{2}]$ = 0.015 M and [ $N O$ ] $=$ 0.025 M.

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Solution

$2 H_{2} + 2 N O \to 2 H_{2} O + N_{2}$

$- \frac{d R}{d t} = k [H_{2}] [N O]^{2}$

$K = 42 M^{- 2} S^{- 1}$ $[H_{2}] = 0.015 M$ $[N O] = 0.025 M$

$- \frac{d R}{d t} = 42 \times 0.015 \times 0.025 = 0.01575$ $M S^{- 1}$

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Similar questions

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

H_{2}

0.42 M^{- 2} s^{- 1}

[H_{2}] = 0.015 M

0.025

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

4.42 M^{- 2} s^{- 1}

[H_{2}] = 0.015 M

2 H_{2}

\to

_{2}

_{2}

H_{2}

M^{- 2}

s^{- 1}

[H_{2}]

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

R a t e = k [H_{2}] [N O]^{2}

2 N O (g) ⇌ N_{2} O_{2} (g)

N_{2} O_{2} + H_{2} \to N_{2} O + H_{2} O

N_{2} O + H_{2} \to H_{2} O + N_{2}

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

{d t [N_{2}] / d t} = k_{1} [N O] [H_{2}]; {d [H_{2} O] / d t) = k [N O] [H_{2}];

{- d [N O] / d t} = k_{1}^{'} [N O] [H_{2}]; {- d [H_{2}] / d t} = k_{1}^{''} [N O] [H_{2}]

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

k_{1}^{''}

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