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 1.60 g H2 is allowed to react with 10.3 g N2, producing 1.48 g NH3. 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 from the chemical equation. 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) HA Value Units Submit Previous Answers Part B 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) Value Units Submit

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 1.60 g H2 is allowed to react with 10.3 g N2, producing 1.48 g NH3. 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 from the chemical equation. 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) HA Value Units Submit Previous Answers Part B 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) Value Units Submit

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

First N2(g) + 3H2(g)—2NH3(g) second NH3(g) + 2O2(g)—HNO3(g) + H2O(g). Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and ox
Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P,(s) + 50,(g) 2 P,0; (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H,PO,): P,0;(g) + 3H,0(1) 2 H;PO, (1) Suppose the yield of the first step is 77.% and the yield of the second step is 67.%. Calculate the mass of phosphorus required to make 6.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Hydrogen fuel can be generated using a process called coal gasification. Hydrogen gas is formed by the reaction of carbon, excess oxygen and excess water. 3C (from coal) + O2 + H2O → H2 + 3CO If this process has an 84.22% yield, what mass of coal (65.5%C by mass) is needed to generate 1.33 kg of hydrogen?
Silicon tetrachloride (SiCl4 ) can be prepared by heating Si in chlorine gas: Si(s) + 2Cl2(g) -> SiCl4(l) In one reaction, 0.507 mole of SiCl4 is produced. What mass (grams) of molecular chlorine were used in the reaction? Choose the nearest answer. MW SiCl4 = 169.9 g/mol; MW Cl = 35.453 g/mol 63 grams 27 grams 72 grams 36 grams
4) Zinc oxide can be produced by the following reaction: 2 Zn (s) + O2(g) 2 ZnO (s) - There are many uses for ZnO, but one is a heat- reflective coating on windows (thus lowering cooling demands in hot climates). This coating requires a thin layer (approximately 40-50 µm thick) of zinc oxide. Assume that this thin film uses 1.9x1020 Zn atoms per cm² of surface. How many grams of ZnO are added to a window that has an area of 5500 cm²? g Zno
Automobile exhaust often contains traces of ethene (C2 H4), which is another possible product of incomplete combustion. Write a balanced equation for the formation of ethene during the combustion of decane. (Water will also be formed as a product.) (Use the lowest possible coefficients. Omit states of matter.) + +
Write a balanced chemical equation based on the following description: solid sodium reacts with chlorine gas to produce solid sodium chloride. Na(s)+Cl2(g)_
Phosgene, a substance used in poisonous gas warfare during World War I, is so named because it was first prepared by theaction of sunlight on a mixture of carbon monoxide and chlorine gases. Its name comes from the Greek words phos (light) andgenes (born of). Phosgene has the following elemental composition: 12.14% C, 16.17% O, and 71.69% Cl by mass. Its molarmass is 98.9 g>mol. (a) Determine the molecular formula of this compound. (b) Draw three Lewis structures for the moleculethat satisfy the octet rule for each atom. (The Cl and O atoms bond to C.) (c) Using formal charges, determine which Lewisstructure is the dominant one. (d) Using average bond enthalpies, estimate ΔH for the formation of gaseous phosgene fromCO(g) and Cl21g2.
How many grams of magnesium oxide can be produced by reacting 0.248 g magnesium that is 97.5% pure with 5.36 x 10^21 molecules oxygen? Write the balanced equation for this reaction.
Write a balanced chemical equation based on the following description: solid cesium reacts with solid cesium nitrite to form cesium oxide and nitrogen gas. The oxidation number of the manganese atom in MnO₄⁻ is The oxidation number of the nitrogen atom in NH₃ is
There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC,(s)+2H,O(g)–C,H,(g)+Ca(OH),(s) In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6 C,H,(g)+3 CO,(9)+4H,0(9)→5 CH,CHCO,H(9) Write the net chemical equation for the production of acrylic acid from calcium carbide, water and carbon dioxide. Be sure your equation is balanced. Explanation Check O 2022 McGraw Hill LLC. AlI Rights Reserved. Terms of Use Privacy Center Accessibility 2:24 PM W 4/8/2022 DELL Esc F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 F12 PrtScr Insert Delete PgUp PgDn Fn C@ 23 2$ Num Lock & Backspace 1 2 3 4 7 8. Co (O
Carborundum (silicon carbide), SiC, is a very hard material used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO2, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. (a) Write the balanced equation for this reaction. (Omit states - of - matter from your answer. Use the lowest possible whole number coefficients.) chemPadHelp (b) Calculate how many kilograms of SiO2 are required to produce 3.14 kg of SIC.