Nitrogen and hydrogen gases are combined at high temperatures and pressures to produce ammonia, NH3. If 100. g of N2 is reacted with excess H2, what number of moles of NH3 will be formed?
Balanced chemical reaction is
N2 + 3H2 2NH3
molar mass of N2 = 28.0134 g/mole
no.of mole = gm of compound / molar mass
mole of N2 = 100 / 28.0134 = 3.5697 mole
According to reaction 1 mole of N2 produce 2 mole of NH3 molar retion of N2 to NH3 = 1:2
therefore 3.5697 mole of N2 produce NH3 = 3.5697 X 2 = 7.14 mole
NH3 will produced = 7.14 mole
Nitrogen and hydrogen gases are combined at high temperatures and pressures to produce ammonia, NH3. If...
Hydrogen gas (H 2 ) and nitrogen gas (N 2 ) combined through the Habes process to produce ammonia gas (NH 3 ) This industrial process occurs at extremely high temperatures and pressures. 3H 2 (g)+N 2 (g) 2NH 3 (g) If 50.9 H 2 combined with excess nitrogen gas and the pressure and temperature are maintained at 201 atm and 460.0 C throughout the reaction, how many grams of ammonia gas will be produced? 3080 113 g g 1930...
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)⟶2NH3(g) Assume 0.200 mol N2 and 0.647 mol H2 are present initially. After complete reaction, how many moles of ammonia are produced? NH3: mol How many moles of H2 remain? H2: mol How many moles of N2 remain? N2: mol
A sample of ammonia (NH3) gas is completely decomposed to nitrogen and hydrogen gases over heated iron wool. If the total pressure is 751 mmHg after the reaction, calculate the partial pressures of N2 and H2. Enter your answers in scientific notation. PN2 × 10 mmHg PH2 × 10 mmHg
26.) Ammonia is produced by the reaction of hydrogen and nitrogen as follows: N2(g)+3H2(g)→2NH3(g)ammonia Express the number of moles to two significant figures. (A.) How many moles of H2 are needed to react with 1.0 mol of N2? (B.) How many moles of N2 reacted if 0.50 mol of NH3 is produced? (C.) How many moles of NH3 are produced when 1.7 mol of H2 reacts?
Ammonia is produced by the reaction of hydrogen and nitrogen as follows: N2(g) + 3H2(g) → 2NH3(g) ammonia You may want to reference (Page) Section 7.6 while completing this problem. Part A How many moles of H2 are needed to react with 0.70 mol of N2? Part B How many moles of N2 reacted if 0.75 mol of NH3 is produced? EPart How many moles of NH3 are produced when 13 mol of H2 reacts ?
Nitrogen gas can be prepared by passing gaseous ammonia over solid CuO at high temperatures. The other products of the reation are solid copper and water vapor. If a sample containing 18.1g of NH3 is reacted with 90.4g of CuO, which is the limiting reactant? How many grams of N2 will be formed? What is the theoretical yield ? If 6.63g are actually producted what is the percent yield in this case? I believe the balanced equation is: 2NH3(g) +...
Nitrogen and hydrogen combine at high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)-->2NH3(g) Assume 4 molecules of nitrogen and 9 molecules of hydrogen are present. After complete reaction, how many molecules of ammonia are produced? How many molecules of H2 remain? How many molecules of N2 remain? What is the limiting reactant?
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)⟶2NH3(g)N2(g)+3H2(g)⟶2NH3(g) Assume 0.280 mol N20.280 mol N2 and 0.880 mol H20.880 mol H2 are present initially. After complete reaction, how many moles of ammonia are produced? Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g) + 3H2(g) + 2NH3(g) Assume 0.280 mol N, and 0.880 mol H, are present initially. After complete reaction, how...
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)⟶2NH3(g) Assume 0.180 mol N2 and 0.564 mol H2 are present initially. How many moles of H2 remain?
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia 2 NH3 (g) N,(g) + 3 Н,(g) — Assume 0.190 mol N, and 0.604 mol H, are present initially After complete reaction, how many moles of ammonia are produced? NH3 mol How many moles of H, remain? Н: mol How many moles of N, remain? N2 mol What is the limiting reactant? Onitrogen O hydrogen