97% 00 Simple Mobile2:20 PM roosevelt.blackboard.com 2. Nitroglycerine decompose
ID: 945328 • Letter: 9
Question
97% 00 Simple Mobile2:20 PM roosevelt.blackboard.com 2. Nitroglycerine decomposes violently according to the chemical equation below. What mass of carbon dioxide gas is produced from the decomposition of 5.00 g C,H(NO),? 4 C3H.(NO( 12 CO (g) + 6N(g) +10 HO(g +O.(g) a. 15.0 g b. 0.969 g c. 11.6g d. 2.91 g e. 0.323 g 3. Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of H,O.? a. 58.8 g b.66.4 g e. 107 g d. 118 g e. 125 g 4. If 15.0 g N2 and 2.00 g H2 react to produce 1.38 g NH, what is the percent yield of the reaction? N2(g)+3 H2(g 2NH,(g) a, 7,57% b. 12.2% C. 8.12% d. 15.1% c. 8.17%Explanation / Answer
2)
m = 5 g of nitroglycerin:
mass of CO2 formed
4 mol of nitroglycerin --> 12 mol of CO2
then
mass of nitroglycerin = 227.0865 g/mol
mol = mass/MW = 5/227.0865 = 0.0220180 mol of nitroglycerin
then, since ratio si 3 to 12; or 1:4
0.0220180*12/3 = 0.088072 mol of CO2
mass of CO2 = mol*MW = 0.088072*44 = 3.875168 g of CO2
3)
H2O= H2 + O2
mass of H2O2 = 125
MW of H2O2 = 34.0147 g/mol
mol = mass/MW = 125/34.0147 = 3.674881
then, since ratio is 1 mol of H2O2 per 1 mol of O2
expect
3.674881 mol of O2
mass of O2 = mol*MW = 3.674881*32 = 117.596192 g of O2
4)
m = 15 g of N2
m = 2 g of H2
m = 1.38 g of NH3
yield ?
yield = real/theoretical * 100
theoretical yield
N2 + 3H2 = 2NH3
mol of H2 = mass/MW = 2/2 = 1
mol of N2 = mass/MW = 17/28 = 0.6071
1 mol of H2 will need 1/3 = 0.33 mol of N", then this is limiting
1 mol of H2 --> 2/3 = 0.666 mol of NH3
mass = mol*MW = 0.666*17 = 11.322 g of NH3
yield = 1.38 /11.322 * 100 = 12.18865 %
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