Q1: A gaseous mixture contains 14 kg of N₂, 16 kg of O₂ and 17 kg of NH₃. The mole fraction of oxygen is

ANS:B - 0.33

To find the mole fraction of oxygen (𝑋O2XO2​​) in the gaseous mixture, we need to first calculate the total number of moles of oxygen and then divide it by the total number of moles of all the gases present in the mixture. Given:

• Mass of O2 = 16 kg
• Molar mass of O2 = 32 g/mol (since oxygen is diatomic)
• Number of moles of O2 = Mass / Molar mass = 16 kg×1000 g/kg32 g/mol=500 mol16kg×32g/mol1000g/kg​=500mol

Now, let's calculate the total number of moles of all gases in the mixture:

• Number of moles of N2 = Mass / Molar mass = 14 kg×1000 g/kg28 g/mol=500 mol14kg×28g/mol1000g/kg​=500mol
• Number of moles of NH3 = Mass / Molar mass = 17 kg×1000 g/kg17 g/mol=1000 mol17kg×17g/mol1000g/kg​=1000mol

Total number of moles = 500 mol (N2500mol (N2​) + 500 mol (O2500mol (O2​) + 1000 mol (NH31000mol (NH3​) = 2000 mol2000mol Now, let's calculate the mole fraction of O2: 𝑋O2=Number of moles of O2Total number of molesXO2​​=Total number of molesNumber of moles of O2​​ 𝑋O2=500 mol2000 mol=0.25XO2​​=2000mol500mol​=0.25 So, the mole fraction of oxygen (𝑋O2XO2​​) in the gaseous mixture is 0.250.25. Therefore, none of the provided options match the calculated value. It seems there might be a mistake in the provided options.