A fuel mixture used in the early days of rocketry contained hydrazine (N_2H_4) a

Question

A fuel mixture used in the early days of rocketry contained hydrazine (N_2H_4) and dinitrogen tetraoxide. When ignited, the mixture released energy and produced elemental nitrogen and water: 2 N_2H_4(I) + N_2O_4(g) rightarrow 3 N_2(g) + 4H_2O(g) [balanced] What is the theoretical yield of elemental nitrogen when 3.12 mols hydrazine and 2.17 mols dinitrogen tetraoxide react? A. 0.723 mol N_2 B. 2.08 mol N_2 C. 4.68 mol N_2 D. 6.52 mol N_2 3. Hydrogen peroxide, H_2O_2, is sold in a dark bottle because it decomposes in the presence of light to form water and oxygen gas. The balanced reaction is 2 H_2O_2 (I) rightarrow 2 H_2O (I) + O_2 (g) [balanced] If 10.0 g H_2O_2 reacts and 4.25 g H2O are formed, what is the percent yield for this reaction? A. 42.5% B. 45.2% C. 80.2% D. 90.4%

Explanation / Answer

limitant reactant is N2H4

then 3.12 mol of N2H4 reacts to form 3/2*3.12 = 4.68 mol of N2

choose C

3.

mol o fH2O2 = mass/MW = 10/34 = 0.294

mol of water = mass/MW = 4.25/18 = 0.236

ratio is 2:2

so

%yield = real /theoretical * 100 =0.236/ 0.294*100 = 80.2721%

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