Hydrazine reacts with O2 according to the following equation:
Hydrazine reacts with O2 according to the following equation:
N2H4(g) + O2(g) → N2(g) + 2H2O(l)
Assume the 02 needed for the reaction is in a 720 L tank at 27.0°C what must the oxygen pressure be in the tank to have enough oxygen to consume 2.47 kg of hydrazine completely?
Pressure = _______ atm
Homework Answers
From ideal gas equation
PV = nRT
From stoichiometric equation number of moles of oxygen required = number of moles of hydrazine reacted = (2.47 × 1000)/32 = 77.1875 moles
Substituting given data , T = 300 K ,
P = 267.4 atm
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Hydrazine, N2H4. emits a large quantity of energy when it reacts with oxygen, which has led to hydrazine's use as a fuel for rockets: N,H4(1) + O2(g) + N2(g) + 2H2O(g) How many moles of each of the gaseous products are produced when 19.6 g of pure hydrazine is ignited in the presence of 19.6 g of pure oxygen? mol N2 mol H2O How many grams of each product are produced? Lg H2O
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Hydrazine, N2H4 has literally been used as rocket fuel. It reacts exothermically with oxygen as shown below: AH=-577 N2H4 (8) + O2(g) →N2 (g) + 2 H2O(g) kJ/mol What quantity of heat is released when 1.00 kg of hydrazine is combusted? 18.0 kJ 6 5.70 x 105 kg 0 1.80 x 10 kg
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