The most important commercial process for converting N₂ from the air into nitrogen-containing compounds is based on the reaction of N2 and H2 to form ammonia (NH3): N2(g) +3 H₂(g) 2 NH, (g) How many moles of NH, can be formed from 3.0 mol of N₂ and 6.0 mol of H₂? Select one OA, 4.0 moles OR. 5.0 males OC 4.5 males OD. 3.5 moles

The most important commercial process for converting N₂ from the air into nitrogen-containing compounds is based on the reaction of N2 and H2 to form ammonia (NH3): N2(g) +3 H₂(g) 2 NH, (g) How many moles of NH, can be formed from 3.0 mol of N₂ and 6.0 mol of H₂? Select one OA, 4.0 moles OR. 5.0 males OC 4.5 males OD. 3.5 moles

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 50A

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A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
Write a balanced equation for the reaction between (a) dihydrogen sulfide and sulfur dioxide gases to form sulfur solid and steam. (b) methane, ammonia, and oxygen gases to form hydrogen cyanide gas and steam. (c) iron(lll) oxide and hydrogen gas to form molten iron and steam. (d) uranium(IV) oxide and hydrogen fluoride gas to form uranium(IV) fluoride and steam. (e) the combustion of ethyl alcohol (C2H5OH) to give carbon dioxide and water.
T Ma M PA USN Be * Ma E Ad G ph ph Do E Un O Ac. 6 Pec O Na O Pe Со Bas 3 Pe Stu "app.101edu.co Question 11 of 11 What is the mass in grams of H2 that can be formed from 55.8 grams of NH3 in the following reaction? 2 NH:(g) → 3 H:(g) + N:(g)
How many grams of Na₂CO3 (molar mass=105.99 g/mol) are formed from the decomposition of 3.75 grams of NaHCO3 molar mass= (84g/mol) according to the following balanced chemical equation. 2NaHCO3+ heat- ---> Na₂CO3 (s) + CO₂(g) + H₂O(g)
5. When 5.0 moles of potassium metal reacts with an excess of H₂0, 3.5 g of H2 are produced. 2 K (s) + 2 H20 (1) 2 KOH (aq) H₂ (g) a. Calculate the number of moles of water needed to react with all of the potassium metal. (Ans: 5 mol) + b. Calculate the theoretical yield of H2, in grams, formed when all 5.0 moles of potassium metal are consumed. (Ans: 5.04 g) c. Calculate the percent yield of the reaction, given 3.5 g (actual yield) are produced. (Ans: 69.4%)
For every one molecule of NaHCO3(s) there is one molecule of CO2(g) that forms: NaHCO3(s) + CH3CO2H(aq) --> CO2(g) + H2O(l) + NaCH3CO2(aq) This means that if we know how many moles of gas we need, we need the same number of moles of sodium bicarbonate to produce it. Now, we need something to fill with gas. I'll be filling a 1-quart sealable plastic bag. 1 quart is 946 mL (0.946 L). We can use the ideal gas law to determine how much gas (in moles) is needed to fill 946 mL. Remember there are four variables for the ideal gas law. Ideal Gas Law: PV = nRT P = pressure: typically 715 mm Hg in Spokane <-- unit dictates which R to use V = volume: 1 quart bag = 0.946 L <-- must be in Liters T = room temperature: 20 °C in my lab, +273 = 293 K <-- must be Kelvin n = moles: what we are solving for I used atmospheric pressure in mm Hg, so I'll have to pick the R value with "mm Hg" in the units: R = 62.4 L × m m H g K × m o l Now, use these values to calculate how many moles of…
Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas (CH4) by the following process: 2NH3(g) + 3O2(g) + 2CH4(g) →PI 2HCN(g) + 6H2O(g) Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reaction vessel contains 11.5 g NH3, 12.0 g O2, and 10.5g CH4, what is the ma_ximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written?
3/5 Yah v Percent yield of chemical reactions Aqueous hydrobromic acid (HBr) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H,0). If 0.997 g of sodium bromide is produced from the reaction of 1.6 g of hydrobromic acid and 1.5 g of sodium hydroxide, calculate the percent yield of sodium bromide. Round your answer to 2 significant figures.
CH3OH can be synthesized by the reaction : CO (g) + 2H2 (g) -----> CH3OH (g) How many liters of CO gas, measured under the same conditions, are required ?
Urea (NH2)2CO) is prepared by reacting ammonia with carbon dioxide according to the equation. 2NH3(g) + CO2(g) ➡ (NH2)CO(s) + H2O(l) In one process, 632.2g of NH3 reacted with 1142g of CO2 Calculate the percentage of nitrogen in urea Will urea be soluble in water? Explain Suggest a possible use for urea
Calcium carbonate decomposes to form carbon dioxide and calcium oxide. CaCO3 --> CO2 + CaO. How many liters of carbon dioxide can 200g of CaCO3 generate?
To produce zinc metal, carbon monoxide reacts with zinc (I1) oxide according to: Zno + CO - Zn + CO2 The carbon monoxide, however, is initially prepared from: 2C+ 02 → 200 How many grams of zinc metal (Zn) may be prepared if If 81.0g of C is used with excess amount of ZnO? Your answer should be numerical and neglect units (e.g., if you calculate 3.5g then input 3.5).

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