For the reaction-2NOg- 2H2g- N2g- 2H2OgThe rate expression can be written in following ways-d-N2-dt-k1-NO-H2- d-H2O-dt-k2-NO-H2- -d-NO-dt-k3-NO-H2- d-H2-dt-k4-NO-N2-The relationship between k1- k2- k3- k4 is-

For the reaction, 2NO(g)+ 2H_2(g)→ N_2(g)+ 2H_2O(g) r_NO2=r_H_22=r_N_21=r_H_2O2 k_3[NO][H_2]2=k_4[NO][H_2]2=k_1[NO][H_2]1=k_2[NO][H_2]2 ∴ k_3=k_4=2k_1=k_2 ...

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Standard VIII

Chemistry

Shortcut-Balancing

For the react...

Question

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 following ways:
$\frac{d [N_{2}]}{d t} = k_{1} [N O] [H_{2}]; \frac{d [H_{2} O]}{d t} = k_{2} [N O] [H_{2}]; \frac{- d [N O]}{d t} = k_{3} [N O] [H_{2}]; \frac{d [H_{2}]}{d t} = k_{4} [N O] [N_{2}]$
The relationship between $k_{1}, k_{2}, k_{3}, k_{4}$ is:

k_{1} = k_{2} = k_{3} = k_{4}

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k_{2} = 2 k_{1} = k_{3} = k_{4}

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k_{2} = 2 k_{3} = k_{1} = k_{4}

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k_{2} = k_{1} = k_{3} = 2 k_{4}

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Solution

The correct option is B $k_{2} = 2 k_{1} = k_{3} = k_{4}$
For the reaction,
$2 N O (g) + 2 H_{2} (g) \to N_{2} (g) + 2 H_{2} O (g)$
$\frac{r_{N O}}{2} = \frac{r_{H_{2}}}{2} = \frac{r_{N_{2}}}{1} = \frac{r_{H_{2} O}}{2}$
$\frac{k_{3} [N O] [H_{2}]}{2} = \frac{k_{4} [N O] [H_{2}]}{2} = \frac{k_{1} [N O] [H_{2}]}{1} = \frac{k_{2} [N O] [H_{2}]}{2}$
$∴ k_{3} = k_{4} = 2 k_{1} = k_{2}$

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Similar questions

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}^{''}

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 between

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

and

k_{1}^{''}

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:

{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}]

The relation ship between

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

and

k_{1}^{''}

is:

Q. For a reaction,

2 N H_{3} ⟶ N_{2} + 3 H_{2}

, it is observed that:

\frac{- d [N H_{3}]}{d t} = k_{1} [N H_{3}], \frac{d [N_{2}]}{d t} = k_{2} [N H_{3}], \frac{d [H_{2}]}{d t} = k_{3} [N H_{3}]

What is the relation between

k_{1}, k_{2}

and

k_{3}

Q. For the reaction

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

- \frac{d [N H_{3}]}{d t} = k_{1} [N H_{3}], \frac{d [N_{2}]}{d t} = k_{2} [N H_{3}], \frac{d [H_{2}]}{d t} = k_{3} [N H_{3}]

then the relation between

k_{1}, k_{2}

and

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is?

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For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g) The rate expression can be written in following ways: d[N2]dt=k1[NO][H2]; d[H2O]dt=k2[NO][H2]; −d[NO]dt=k3[NO][H2]; d[H2]dt=k4[NO][N2] The relationship between k1, k2, k3, k4 is:

The correct option is B k2=2k1=k3=k4For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g) rNO2=rH22=rN21=rH2O2 k3[NO][H2]2=k4[NO][H2]2=k1[NO][H2]1=k2[NO][H2]2 ∴k3=k4=2k1=k2