$9.2 g$ of $N X_{2} O X_{4}$ (N = 14, O = 16) is vaporised and partly dissociates, $N X_{2} O X_{4} 2 NO X_{2}$ . The mean molar mass of the resulting gas mixture is $69.0 g mo l^{- 1}$ . Find the mass of $NO X_{2}$ present, in grams, to two decimals.

Numerical answer type, answer in g, tolerance 0.01.

Answer: 3.07 g

Start with 0.100 mol N2O4. Mean M = 92/(1 + alpha), so 1 + alpha = 92/69 = 1.3333 and alpha = 0.3333. NO2 formed = 2 x 0.100 x alpha = 0.0667 mol. Mass = 0.0667 x 46 = 3.07 g.

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9.2 g of NX2​OX4​ (N = 14, O = 16) is vaporised and partly dissociates, NX2​OX4​​2NOX2​. The mean molar mass of the resulting gas mixture is 69.0 g mol−1. Find the mass of NOX2​ present, in grams, to two decimals.

Answer: 3.07 g

More questions on Average molar mass of mixtures, vapour density

$9.2 g$ of $N X_{2} O X_{4}$ (N = 14, O = 16) is vaporised and partly dissociates, $N X_{2} O X_{4} 2 NO X_{2}$ . The mean molar mass of the resulting gas mixture is $69.0 g mo l^{- 1}$ . Find the mass of $NO X_{2}$ present, in grams, to two decimals.