An organic compound contains only carbon, hydrogen, and nitrogen. Complete combustion of 0.288 g of this compound produces 0.88 g of CO ₂ and 0.18 g of H ₂ O . When the same mass of the compound is subjected to Duma's method, it produces 24.6 mL of nitrogen gas collected over water at 300 K and 775 mmHg pressure. If the empirical formula of the compound is C _ x H _ y N _ z (where x, y, z are the simplest whole numbe

Step-by-step solution

Moles of carbon = Moles of CO ₂ = 0.88 44 = 0.02 mol Moles of hydrogen = 2 Moles of H ₂ O = 2 0.18 18 = 0.02 mol For nitrogen estimation by Duma's method: Pressure of dry N ₂ gas = 775 - 15 = 760 mmHg = 1 atm Moles of N ₂ gas, n = PV RT = 1 0.0246 0.082 300 = 0.001 mol Moles of nitrogen atoms = 2 0.001 = 0.002 mol Molar ratio of C : H : N = 0.02 : 0.02 : 0.002 = 10 : 10 : 1 The empirical formula is C ₁₀ H ₁₀ N . Thus, x = 10 , y = 10 , z = 1 . Value of (x + y + z) = 10 + 10 + 1 = 21 . Answer: 21