For the reaction 2N2O5(g) xrightarrow[]4NO2(g)+O2(g) if the concentration of NO2 increases by 5.2× 10-3 M in 100 s then the rate of the reaction is:

Question

For the reaction 2N2O5(g) xrightarrow[]4NO2(g)+O2(g) if the concentration of NO2 increases by 5.2× 10-3 M in 100 s then the rate of the reaction is: (A)  1.3× 10-5Ms-1  (B)  0.5× 10-4Ms-1  (C)  7.6× 10-4Ms-1  (D)  2× 10-3Ms-1

Tardigrade Admin · Accepted Answer

Rate of reaction =(1/4)(d(NO2)/dt) = (5.2× 10-3/4× 100) =1.3× 10-5Ms-1

Q. For the reaction
$2 N_{2} O_{5} (g) 4 N O_{2} (g) + O_{2} (g)$
if the concentration of $N O_{2}$ increases by $5.2 \times 10^{- 3}$ M in 100 s then the rate of the reaction is:

$1.3 \times 10^{- 5} M s^{- 1}$

$0.5 \times 10^{- 4} M s^{- 1}$

$7.6 \times 10^{- 4} M s^{- 1}$

$2 \times 10^{- 3} M s^{- 1}$

$2.5 \times 10^{- 5} M s^{- 1}$

Rate of reaction $= \frac{1}{4} \frac{d ( N O _{2} )}{d t}$
= $\frac{5.2 \times 10 ^{- 3}}{4 \times 100}$
$= 1.3 \times 10^{- 5} M s^{- 1}$

Q. For the reaction 2N2​O5​(g)​4NO2​(g)+O2​(g) if the concentration of NO2​ increases by 5.2×10−3 M in 100 s then the rate of the reaction is:

1.3×10−5Ms−1

0.5×10−4Ms−1

7.6×10−4Ms−1

2×10−3Ms−1

2.5×10−5Ms−1

Rate of reaction =41​dtd(NO2​)​ = 4×1005.2×10−3​ =1.3×10−5Ms−1