Answer: 1.80 x 104 kJ
Hydrazine, N2H4 has literally been used as rocket fuel. It reacts exothermically with oxygen as shown...
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
15. (10 pts.) Hydrazine (N2H) is commonly used as rocket fuel. It reacts with oxygen according to the balanced chemical equation: N2H4(g) + 302(g) + 2N02(g) + 2H20(1) Compound Molecular Weight (g/mol) 70.5 g of Hydrazine (N2Ha) is reacted with 195.3 g of Oz to test | N₂H4 32.06 the thermodynamics of the reaction. 02 32.00 MAKE SURE TO SHOW ALL OF YOUR WORK 46.01 NO a. Identify the limiting reactant:
Hydrazine, N2H4 , reacts with oxygen to form nitrogen gas and water. N2H4(aq)+O2(g)⟶N2(g)+2H2O(l) If 4.05 g of N2H4 reacts with excess oxygen and produces 0.750 L of N2 , at 295 K and 1.00 atm, what is the percent yield of the reaction?
15. (10 pts.) Hydrazine (N,Ha) is commonly used as rocket fuel. It reacts with oxygen according to the balanced chemical equation: N2H4(g) + 302(g) + 2N02(g) + 2H20(1) 70.5 g of Hydrazine (N,Ha) is reacted with 195.3 g of Oz to test the thermodynamics of the reaction. MAKE SURE TO SHOW ALL OF YOUR WORK Compound Molecular Weight (g/mol) N2H4 32.06 0 32.00 NOZ 46.01 a. Identify the limiting reactant: b. How many grams of NO, should be produced in...
hydrazine N2H4 reacts with oxygen to form nitrogen gas and water Hydrazine, N, H, reacts with oxygen to form nitrogen gas and water. N,H, (aq) +0,6) N,(g) + 2 H2O(1) If 2.45 g of N, H, reacts with excess oxygen and produces 0.950 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? percent yield:
Hydrazine, N2H4, may react with oxygen to form nitrogen gas and water. N2H4(aq) + O2(g) -> N2(g) + 2H2O(l) If 3.45 g of N2H4 reacts and produces 0.350 L of N2, at 295 K and 1.00 atm, what is the percent yield of the reaction?
Hydrazine, N2H4N2H4, reacts with oxygen to form nitrogen gas and water. N2H4(aq)+O2(g)⟶N2(g)+2H2O(l)N2H4(aq)+O2(g)⟶N2(g)+2H2O(l) If 2.55 g2.55 g of N2H4N2H4 reacts with excess oxygen and produces 0.550 L0.550 L of N2N2, at 295 K295 K and 1.00 atm,1.00 atm, what is the percent yield of the reaction?
Hydrazine, N2H4N2H4, reacts with oxygen to form nitrogen gas and water. N2H4(aq)+O2(g)⟶N2(g)+2H2O(l)N2H4(aq)+O2(g)⟶N2(g)+2H2O(l) If 2.05 g2.05 g of N2H4N2H4 reacts with excess oxygen and produces 0.650 L0.650 L of N2N2, at 295 K295 K and 1.00 atm,1.00 atm, what is the percent yield of the reaction?
Hydrazine (N2H4) is a liquid that burns in oxygen gas to yield nitrogen gas and water vapor. Using the data below, determine the ΔG and the equilibrium constant for the combustion reaction. Chemical ΔGfº (kJ/mol): [N2 (g)=0] [N2H4 (l)=149] [N2H4 (g)=159] [H2O (l)=-237] [H2O (g)=-229] [O2(g)=0] I got that ΔG is -607, but why does K=e^245?
Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4according to this equation: N2H4(l)+N2O4(g)→2N2O(g)+2H2O(g) Standard Enthalpies of Formation at 25 ∘C Substance ΔH∘f(kJ/mol) N2H4(l) 50.6 N2H4(g) 95.4 N2O(g) 81.6 N2O4(l) −19.5 N2O4(g) 9.16 H2O(l) −285.8 H2O(g) −241.8 Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. Express your answer using one decimal place.