N2O4 (l) + 2 N2H4 (l) → 3 N2 (g) + 4 H2O (g)
Determine the mass (in g) of nitrogen gas that can be formed from 50.0 g dinitrogen...
Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N 2O 4 and 45.0 g N 2H 4. Some possibly useful molar masses are as follows: N 2O 4 = 92.02 g/mol, N 2H 4 = 32.05 g/mol. N 2O 4( l) + 2 N 2H 4( l) → 3 N 2( g) + 4 H 2O( g) LR = N2O4, 45.7 g N2 formed LR = N2O4, 105 g...
The reaction of hydrazine with dinitrogen tetroxide has the following unbalanced equation N2H4 + N2O4 N2 + H2O The coefficient for nitrogen gas in the balanced equation is...
50.0 g N2O4 reacts with 45.0 g N2H4. Determine the percent yield if 12.5 g of N2 are actually formed. N2O4(l) + 2N2H4(l) ---> 3N2(g) + 4H2O(g)
A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetroxide (N2O4) which ignite on contact to form nitrogen gas and water vapor. How many grams of nitrogen gas form when 1.00 x 10^2 g of N2H4 and 2.00 x 10^2 g of N2O4 are mixed? So, I tried solving this but not sure what they mean by "mixed". The balanced chemical equation is: 2 N2H4 + N2O4 = 3 N2 +...
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?
mttps://www.o... Student Cons... Diagnostic Re... Quiz: E D Question 55 1 pts Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N204 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N H4 = 32.05 g/mol. N2O4(1) + 2 N2H4(1) 3 N2(g) + 4H2O(g) OLR-N2H4, 59.0 g N formed OLR-N204, 105 g Ny formed No LR, 45.0 g N2formed OLR-N2H4, 13.3 g N...
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, 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?
Hydrazine, N2H4, may react with oxygen to form nitrogen gas and water. If 3.95 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?
35 and 36 thank you QUESTION 35 Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N204 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N204 = 92.02 g/mol, N2H4 = 32.05 g/mol. N204(0) + 2 N2H40 →3N2(g) + 4H2O(9) O LR = N2H4, 59.0 g N2 formed O No LR, 45.0 g N2 formed O LR = N2H4, 13.3 g N2 formed O LR =...