In a reaction- N 2 O 5 - 2N O 2 - 1 2 O 2- the rate of disappearance of N 2 O 5 is 6-5- 10 -3 mol L -1 s -1- Compute the rates of formation of N O 2 and O 2-

d[ N _ 2 O _ 5 ] #160; dt = 1 2 d[ NO _ 2 ] #160; dt = 1 2 d[ O _ 2 ] #160; dt 6.5× 10 ^ 3 = 1 2 d[ NO _ 2 ] #160; dt = 1 ...

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Nernst Equation

In a reaction...

Question

In a reaction, $N_{2} O_{5} \to 2 N O_{2} + \frac{1}{2} O_{2}$ , the rate of disappearance of $N_{2} O_{5}$ is $6.5 \times 10^{- 3}$ $m o l$ $L^{- 1} s^{- 1}$ . Compute the rates of formation of $N O_{2}$ and $O_{2}$ .

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N_{2} O_{5}

N_{2} O_{5} ⟶ 2 N O_{2} + \frac{1}{2} O_{2}

N_{2} O_{5}

1.8 \times 10^{- 3}

m o l

{l i t r e}^{- 1}

{m i n}^{- 1}

N O_{2}

O_{2}

2 N_{2} O_{5} ⟶ 4 {N O}_{2} + O_{2}

3.0 \times 10^{- 4} s^{- 1}

1.0

m o l

L^{- 1}

N_{2} O_{5}

{N O}_{2}

O_{2}

0.1 m o l

L^{- 1}

2 {N O}_{2} ⟶ N_{2} O_{2} + O_{2}

- \frac{d [{N O}_{2}]}{d t} = k {[{N O}_{2}]}^{n}

k = 3 \times 10^{- 3} {m o l}^{- 1} L {s e c}^{- 1}

1.5 \times 10^{- 4} m o l L^{- 1} {s e c}^{- 1}

{N O}_{2}

L^{- 1}

N_{2} O_{5} ⟶ 2 N O_{2} + 1 / 2 O_{2}

- \frac{d [N_{2} O_{5}]}{d t} = k_{1} [N_{2} O_{5}]

\frac{d [N O_{2}]}{d t} = k_{2} [N_{2} O_{5}]

\frac{d [O_{2}]}{d t} = k_{3} [N_{2} O_{5}]

k_{1}, k_{2}

k_{3}

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