21. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the following equation 3 H2 (g) + N2 (g) → 2 NH3 (g) The production of ammonia is difficult and often results in lower yields than those predicted from the chemical equation. For instance, if 1.36 g of hydrogen gas are allowed to react with 9.97 g of nitrogen gas, 2.24 g of ammonia are produced. What is the theoretical yield of the reaction? а. 11.5 g b. 2.24 g с. 7.66 g d. 6.06 g

21. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the following equation 3 H2 (g) + N2 (g) → 2 NH3 (g) The production of ammonia is difficult and often results in lower yields than those predicted from the chemical equation. For instance, if 1.36 g of hydrogen gas are allowed to react with 9.97 g of nitrogen gas, 2.24 g of ammonia are produced. What is the theoretical yield of the reaction? а. 11.5 g b. 2.24 g с. 7.66 g d. 6.06 g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A reinforced steel cylinder is filled with 21.0 moles of hydrogen and 12.0 moles of oxygen. The mixture is detonated inside the cylinder causing the following reaction to take place. 2 H2(g) + O2(g) → 2 H2O (g) What is the theoretical yield, in grams, of the reaction?
How many moles of Al are necessary to form 28.6 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s) ?
48
The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation 3H₂(g) + N₂ (g)→2NH3(g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals. However, the production of ammonia is difficult, resulting in lower yields than those predicted the chemical equation. 1.56 g H₂ is allowed to react with 10.1 g N₂, producing 2.25 g NH3. Part A What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) Value Submit Part B μÃ Submit What is the percent yield for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) μĂ Value Units Units ? wwwww ?
Barium hydride reacts with water to produce barium hydroxide and hydrogen gas. BaH₂ (s) + 2 H₂O(1)→ Ba(OH)2 (aq) + H₂(g) If 6.389 g BaH2 is combined with 64.000 g H₂O, the reaction proceeds until all the BaH₂ is consumed. The hydrogen gas escapes to the environment, and the final weight of the flask is 70.204 g. The remaining water is evaporated, leaving 7.856 g Ba(OH)2. What mass of water is consumed in the reaction? g H₂O BO esc :0 F1 2 1086 TeTWE F2 # OCT 3 3 80 F3 $ 4 F4 R 65 % F5 T COMING MacBook Pro < 6 F6 Y & A 7 aa F7 * 00 U 8 DII F8 tv A S I F9 2 S F10 0 0 Save and Exit a F11
Lead(II) oxide from an ore can be reduced to elemental lead by heating in a furnace with carbon. Calculate the expected yield of lead if 67.0 kg of lead oxide is heated with 67.0 kg of carbon.
The reaction of 1.0 gram of aluminum (Al) and 1.0 gram of oxygen (O2) according to the reaction below produced 1.7 grams of aluminum oxide (Al2O3). 4 Al (s) + 3 O2 (g) → 2 Al2O3 (s) Calculate the theoretical yield of aluminum oxide
Prior to their phaseout in the 1980s, chemicals containing lead were commonly added to gasoline as anti-knocking agents. A 4.887 g sample of one such additive containing only lead, carbon, and hydrogen was burned in an oxygen-rich environment. The products of the combustion were 5.319 g CO2(g) and 2.722 g H2O(g). Determine the empirical formula of the gasoline additive.
During a laboratory experiment, a student initiated a reaction with 19.5 g of NaBH4 and excess BF3. When the reaction was complete, the student had collected 7.00 g of B2H6 gas. From this data, calculate the percent yield of B2H6.
The balanced chemical equation is 8 Al₂S₃(s) → 16 Al(s) + 3 S₈(s). How many moles of Al can be formed from the decomposition of 1.62 moles of the reactant based on the balanced chemical equation?
Consider the balanced chemical equation when 18.3 g Al is reacted with 113 g I₂ to form AlI₃(g). a. Calculate the theoretical yield in grams AlI₃ from the complete reaction of 18.3 grams Al according to the following balanced chemical equation: 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) b. Calculate the theoretical yield in grams AlI₃ from the complete reaction of 113 grams I₂ according to the following balanced chemical equation: 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) c. Which of the following substances is the limiting reactant? 2 Al(s) + 3 I₂(g) → 2 AlI₃(g) d. What is the mass in grams of the excess Al remaining after the partial reaction of 18.3 g Al with 113 g I₂? 2 Al(s) + 3 I₂(g) → 2 AlI₃(g)
Consider the reaction 3X + 2Y → 5C + 4D How many moles of X are needed to produce 23.00 moles of D?