In 2N2O5 -> 4NO2 + O2 (molar masses: NO2 = 46, N2O5 = 108 g mol^-1), NO2 is formed at 2.76 g L^-1 s^-1. What mass of N2O5 (in g) is consumed per litre per minute? Give the answer to one decimal place.

JEE Advanced levelNumerical answerDifficulty 3 of 3ck198

In $2 N X_{2} O X_{5} 4 NO X_{2} + O X_{2}$ (molar masses: $NO X_{2}$ = 46, $N X_{2} O X_{5}$ = 108 $g mo l^{- 1}$ ), $NO X_{2}$ is formed at $2.76 g L^{- 1} s^{- 1}$ . What mass of $N X_{2} O X_{5}$ (in g) is consumed per litre per minute? Give the answer to one decimal place.

Numerical answer type, answer in g/L/min, tolerance 0.1.

Rate of

NO X_{2}

formation

= 2.76/46 = 0.060 M s^{- 1}

. Since

- \frac{1}{2} d [N X_{2} O X_{5}] / d t = \frac{1}{4} d [NO X_{2}] / d t

N X_{2} O X_{5}

is lost at

0.060/2 = 0.030 M s^{- 1} = 1.80 M mi n^{- 1}

. Mass =

1.80 \times 108 = 194.4 g L^{- 1} mi n^{- 1}