Hydrazine reacts with O2 according to the followingequation: N2H4(g) + O2(g) ---

Question

Hydrazine reacts with O2 according to the followingequation: N2H4(g) + O2(g) ----> N2(g) + 2 H2O Assume the O2 needed for the reaction is in a 450-L tank at 23deg. C. What must the oxygen pressure be in the tank to have enoughoxygen to consumre 1.00 kg of hydrazine completely? I need step by step process pls.     ans.in back of the book has 1.7 atm O2 Hydrazine reacts with O2 according to the followingequation: N2H4(g) + O2(g) ----> N2(g) + 2 H2O Assume the O2 needed for the reaction is in a 450-L tank at 23deg. C. What must the oxygen pressure be in the tank to have enoughoxygen to consumre 1.00 kg of hydrazine completely? I need step by step process pls.     ans.in back of the book has 1.7 atm O2

Explanation / Answer

N2H4(g) + O2(g) ----> N2(g) + 2 H2O Molar mass of N2H4 is = 2 * 14 + 4 * 1 = 32 g / mol Molar mass of O2 is = 2 * 16 = 32 g 32 g of Hydrazine reacts with 32 g of O2 So 1Kg of Hydrazine reacts with 1Kg of O2 So the mass of O2 reacted m = 1 Kg = 1000 g We know that PV = nRT                             =( m / M ) RT Where m = mass of O2 = 1000 Kg P = Pressure = ? V = Volume of O2 = 450 L ( since the volume of the gas =Volume of the tank ) M = Molar mass of O2 = 32 g / mol R = gas constant = 0.0821 L atm / mol - K T = Temperature = 23 oC = 23+273 = 296 K Plug the values we get P = mRT / MV                                      = 1.6876 atm                                      ~ 1.7 atm of O2

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