Question 4 of 15SubmitDetermine the number of grams of CaH10 that are required to completely react toproduce 8.70 mol of CO2 according to the following combustion reaction:2C.H10(g) +13 O:(g)8CO:(g) +10H:O(g)STARTING AMOUNTADD FACTORANSWERRESET*( )28.706.022 x 10232.180.037444.014.35208.001318.021261058.141g O.g H2Og CO2mol CO2mol O2mol CAH10mol H2Og CH10

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Answered: Question 4 of 15 Submit Determine the…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 161IP: In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric...

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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.
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.
In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H+(aq)+NO3(aq)+UO2+(aq)NO(g)+UO22+(aq)+H2O(l) If 2.55 102 mL NO(g) is isolated at 29C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
One way to remove nitrogen oxide (NO) from smoke-stack emissions is to react it with ammonia. 4NH3(g)+6NO(g)5N2(g)+6H2O(l) Calculate (a) the mass of water produced from 0.839 mol of ammonia. (b) the mass of NO required to react with 3.402 mol of ammonia. (c) the mass of ammonia required to produce 12.0 g of nitrogen gas. (d) the mass of ammonia required to react with 115 g of NO.
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
Limestone rocks are composed mainly of calcium carbonate (CaCO3) that reacts easily with a hydrochoric acid, releasing carbon dioxide gas. Find the following: a. Show the balanced chemical equation. b.Based on the balanced equation (in a), how much CO2 (in L) will be produced by 250 g of CaCO3 if it is completely reacted with HCl at 25°C and 1.0 atm? c.Based on the reaction, is it safe to use muriatic acid to clean limestone tiles? Explain.
The combustion of gasoline produces carbon dioxide andwater. Assume gasoline to be pure octane (C8H18) and calculatehow many kilograms of carbon dioxide are added tothe atmosphere per 1.0 kg of octane burned. (Hint: Begin bywriting a balanced equation for the combustion reaction.)
Ethylene burns in oxygen to form carbon dioxide and water vapor: C2H4(g)+ 3 O2(g)-->2 CO2(g)+ 2 H2O(g) How many liters of water can be formed if 1.25 liters of ethylene are consumed in this reaction? (Assume STP) L H2O (3 sig figs)
A 10.0-g sample of C2H5OH is burned completely in air. How many moles of H2O are formed?
How many moles of O2 will form when 1.818 moles of CO2 react with 3.583 moles of KO2? Enter your answer to the thousandths place. Do not include units. 4KO2(s) + 2CO2(g) ⟶ 2K2CO3(s) + 3O2(g)
How many moles of H2O2 are needed to produce 3.90 mol of H2O?

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