For the reaction, N2 O5 (g) longrightarrow 2NO2 (g) +(1/2) O2 (g) The value of rate of disappearance of N2 O5 is given as 6.25 x 10-3 mol L-1 s-1. The rate of formation of NO2 and O2 is given respectively as

Question

For the reaction, N2 O5 (g) longrightarrow 2NO2 (g) +(1/2) O2 (g) The value of rate of disappearance of N2 O5 is given as 6.25 x 10-3 mol L-1 s-1. The rate of formation of NO2 and O2 is given respectively as (A) 6.25 x 10-3 mol L-1 s-1 and 6.25 × 10-3 mol L-1 s-1 (B) 1.25 x 10-2 mol L-1 s-1 and 3.125 × 10-3 mol L-1 s-1 (C) 6.25 x 10-3 mol L-1 s-1 and 3.125 × 10-3 mol L-1 s-1 (D) 1.25 x 10-2 mol L-1 s-1 and 6.25 × 10-3 mol L-1 s-1

Tardigrade Admin · Accepted Answer

Key Idea Rate of disappearance of reactant = rate of appearance of product

or

- \frac{1}{Stoichiometric coefficient of reactant} \frac{d [ reactant ]}{d t}

= + \frac{1}{Stoichiometric coefficient of product} \frac{d [ product ]}{d t}

For the reaction,

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

\frac{- d [ N _{2} O _{5} ]}{d t} = + \frac{1}{2} \frac{d [ N O _{2} ]}{d t}

∴ \frac{d [ N O _{2} ]}{d t} = - 2 \frac{d [ N _{2} O _{5} ]}{d t}

= 2 \times 6.25 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}

= 12.5 \times 1 0^{- 3} m o l L - 1 s^{- 1}

= 1.25 \times 1 0^{- 2} m o l L - 1 s^{- 1}

\frac{d [ O _{2} ]}{d t} = - \frac{d [ N _{2} O _{5} ]}{d t} \times \frac{1}{2}

= \frac{6.25 \times 1 0 ^{- 3} m o l L ^{- 1} s ^{- 1}}{2}

= 3.125 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}

Q. For the reaction, $N_{2} O_{5 (g)} ⟶ 2 N O_{2 (g)} + \frac{1}{2} O_{2 (g)}$ The value of rate of disappearance of $N_{2} O_{5}$ is given as 6.25 x $1 0^{- 3} m o l L^{- 1} s^{- 1}$ . The rate of formation of $N O_{2}$ and $O_{2}$ is given respectively as

6.25 x $1 0^{- 3} m o l L^{- 1} s^{- 1} an d 6.25 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

1.25 x $1 0^{- 2} m o l L^{- 1} s^{- 1} an d 3.125 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

6.25 x $1 0^{- 3} m o l L^{- 1} s^{- 1} an d 3.125 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

1.25 x $1 0^{- 2} m o l L^{- 1} s^{- 1} an d 6.25 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

Q. For the reaction, N2​O5(g)​⟶2NO2(g)​+21​O2(g)​ The value of rate of disappearance of N2​O5​ is given as 6.25 x 10−3molL−1s−1. The rate of formation of NO2​ and O2​ is given respectively as

6.25 x 10−3molL−1s−1and6.25×10−3molL−1s−1

1.25 x 10−2molL−1s−1and3.125×10−3molL−1s−1

6.25 x 10−3molL−1s−1and3.125×10−3molL−1s−1

1.25 x 10−2molL−1s−1and6.25×10−3molL−1s−1

Q. For the reaction, $N_{2} O_{5 (g)} ⟶ 2 N O_{2 (g)} + \frac{1}{2} O_{2 (g)}$ The value of rate of disappearance of $N_{2} O_{5}$ is given as 6.25 x $1 0^{- 3} m o l L^{- 1} s^{- 1}$ . The rate of formation of $N O_{2}$ and $O_{2}$ is given respectively as

6.25 x $1 0^{- 3} m o l L^{- 1} s^{- 1} an d 6.25 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

1.25 x $1 0^{- 2} m o l L^{- 1} s^{- 1} an d 3.125 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

6.25 x $1 0^{- 3} m o l L^{- 1} s^{- 1} an d 3.125 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$

1.25 x $1 0^{- 2} m o l L^{- 1} s^{- 1} an d 6.25 \times 1 0^{- 3} m o l L^{- 1} s^{- 1}$