Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) → 2NH3(g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH3(g) + 20₂(g) HNO3(g) + H₂O(g) Suppose the yield of the first step is 95.% and the yield of the second step is 83.%. Calculate the mass of hydrogen required to make 4.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 0 nln X ロ・ロ 3

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) → 2NH3(g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH3(g) + 20₂(g) HNO3(g) + H₂O(g) Suppose the yield of the first step is 95.% and the yield of the second step is 83.%. Calculate the mass of hydrogen required to make 4.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 0 nln X ロ・ロ 3

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...

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Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3 H₂(g) → 2 NH3(g) ΔΗ= - 92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g) + 2O₂(g) → HNO3(g) + H₂O(g) ΔΗ= - 330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. ☐ kJ X 3
O = rosoft C W There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(1) oxide and sulfur dioxide: 2Cu₂S (s) + 30₂(g) → 2Cu₂0(s) + 2 SO₂ (g) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu₂O(s) + C(s)→ 2Cu(s) + CO (g) Microsoft O CHEMICAL REACTIONS Reaction sequence stoichiometry Microsoft 6.52.210... esc Suppose the yield of the first step is 64.% and the yield of the second step is 88.%. Calculate the mass of oxygen required to make 2.0 kg of copper. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. Explanation aption Q A T N 11 2 Check 9,039 W S X command #3 E 010 14 4 X $ C DEC 3 R F Ś % 5 V T útv G () > Y Ø 7 H Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibil 917 C N * 00 8 J FERBARKE I A M -0 K O L 28 W command
1. What is the final overall reaction for these three reactions below? Reaction 1: C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g), AHị = -2043 kJ Reaction 2: C (s) + O2 (g) Reaction 3: 2 H2 (g) + O2 (g) + CO2 (g), AH2 = -393.5 kJ → 2 H2O (g), AH3 = -483.6 kJ Hint. Reverse Reaction 1 then simplify by cancelling compounds in opposite sides of the arrow. 2. What is the AHorxn for the reaction in kJ?
The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine molecule consumed [2 Na(s) + Cl2(g) → 2 NaCl(s)]. How much heat is released (in kJ) if 1.569 g of Na are consumed in the reaction?
a. Hydrogen cyanide is used in the manufacture of clear plastics such as Lucite and Plexiglas. It is prepared from ammonia and natural gas (CH4). 2NH3 (g) + 302 (9) + 2CH4 (g) → 2HCN(g) + 6H2O The reaction evolves 939 kJ of heat per 2 mol HCN formed. Is the reaction endothermic or exothermic? endothermic exothermic b. If 8 mol of HCN is produced, what is the value of q? kJ
Consider the following reaction. (a) Is the reaction exothermic or endothermic? exothermic endothermic CH3OH(g) → CO(g) + 2 H₂(g) AH +90.7 kJ (b) Calculate the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. ΔΗ= 100.8 (c) If the enthalpy change is 19.0 kJ, how many grams of hydrogen gas are produced? 0.42 x g (d) How many kilojoules of heat are released when 13.0 g of CO(g) reacts completely with H₂(g) to form CH₂OH(g) at constant pressure? AH = -90.7 X kJ (e) Calculate AE when 400.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol K-41.7 XkJ HopHelpCh5N1
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The reaction between sodium metal and chlorine gas produces 822 kJ of heat energy for every chlorine molecule consumed [2 Na(s) + Cl2(g) → 2 NaCI(s)]. How much heat is released (in kJ) if 4.785 g of Na are consumed in the reaction?
4. You wish to determine the amount of heat produced by the reaction of propane with oxygen. You are given some known reactions: I. II. III. 3 C(s) (g) + 4H₂(g) → C₂H₂ (g) C(s) (g) + O₂(g) → CO₂ (g) H₂(g) + O₂(g) → H₂O (1) ΔΗ, ΔΗ, ΔΗ, (a) Combine reactions 1, 2 and 3 to form a series of steps that sum to the combustion of propane: C₂H₂(g) +50₂ (g) →3CO₂ (g) + 4H₂O (1) (b) Given the following values for the enthalpy changes, combustion of propane. AH₂=-393.5 kJ/mol AH, =-103.85 kJ/mol calculate AH for the AH, = -285.8kJ/mol
How many mole is present in the reactant and product in the given belwo
If 2C4H10 + 13O2 --> 8CO2 + 1OH2O is exothermic, is energy (heat) a reactant or product?
Train track rails are joined using an exothermic welding process. A mixture of iron (III) oxide (Fe2O3), and aluminium metal (Al) is employed and the process is described by the following chemical reaction: Fe₂O3(s) + 2Al(s) → Al₂O3(s) + 2Fe(s) AH (kJ mol-1) c(g-¹ K-1) 0 0.451 Fe(s) Fe₂O3(s) -822.3 0.651 0 0.900 Al(s) Al2O3(s) -1669.8 0.753 a) Calculate the heat released by this process. b) Assuming the reaction goes to completion and that all the heat goes into the final mixture, calculate the final temperature of the products before heat has flowed into the surroundings. Comment on whether the calculated temperature is reasonable. c) Calculate the entropy change for the surroundings once the system and surroundings have equilibrated to the surrounding temperature of 25 °C.