When the following equations are balanced using smallest integers, what is the coefficient O2 or H2? a) C8H18(l) + O2(g) → CO2(g) + H2O(g) Coefficient of O2 = b) CH3OH(l) + O2(g) → CO2(g) + H2O(g) Coefficient of O2 = c) NH3(l) + O2(g) → NO(g) + H2O(g) Coefficient of O2 = d) Fe(s) + HCl(aq) → FeCl3(aq) + H2(g) Coefficient of H2 =

When the following equations are balanced using smallest integers, what is the coefficient O2 or H2? a) C8H18(l) + O2(g) → CO2(g) + H2O(g) Coefficient of O2 = b) CH3OH(l) + O2(g) → CO2(g) + H2O(g) Coefficient of O2 = c) NH3(l) + O2(g) → NO(g) + H2O(g) Coefficient of O2 = d) Fe(s) + HCl(aq) → FeCl3(aq) + H2(g) Coefficient of H2 =

Chemistry for Engineering Students

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Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.50PAE: 3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of...

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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.
3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of operation. How many moles of NO2 would this engine release if it were used for a 45-minute commute, assuming that this mea- sured number is representative of the emission under all circumstances?
When the equation H2 + Fe + H2O is completely balanced with the smallest whole numbers, the coefficient of H2 would be
Burning coal that contains sulfur releases sulfur dioxide gas into the atmosphere where it combines with water to form sulfurous and sulfuric acid, thereby producing acid rain. Assume sulfur in coal is in the form of pyrite (FeS2(s)), which reacts with molecular oxygen to produce Fe2O3(s) and SO2(g). Write the balanced equation for this reaction and report the sum of the stoichiometric coefficients, written as integers.
Balance the following equations. (Use the lowest coefficients.) (a) C3H8 + O2 CO2 + H2O(b) Fe2O3 + C Fe + CO(c) C4H8 + O2 CO2 + H2O
Given the chemical equation C4H10 + O2 ⟶ ⟶ CO2 + H2O, what coefficient is needed in front of C4H10 to produce a balanced equation?
Isoamyl acetate, C7H14O2, is used to flavor banana candies. Write and balance the chemical equation for the combustion of isoamyl acetate. Calculate the molar mass of isoamyl acetate. How many grams of carbon dioxide is formed from 65.23 g of isoamyl acetate? Report your final answer with the proper significant figures.
Given (8.79x10^6) moles of glucose, C6H12O6, calculate the mole of carbon dioxide, CO2, formed upon complete oxidation of the glucose. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O Express your answer in three significant digits as moles. Note: Your answer is assumed to be reduced to the highest power possible.
When the equation __C2H6 + __O2 --------> __CO2 + __H2O is correctly balanced using the smallest whole number coefficients, the sum of the coefficients is
SO2 is a product of coal combustion. It may combine with O2 and H2O in the atmosphere to form sulfuric acid, a component of acid rain. One way to reduce the formation of acid rain involves trapping the SO2 by passing smokestack gases through a spray of calcium oxide and O2. The product of this reaction is calcium sulfate. a) Write a balanced chemical equation describing this reaction by writing the product and adding coefficients. __SO2+__CaO+__O2=__CaSO4 b) How many metric tons of calcium sulfate would be produced from each metric ton of SO2 that is trapped?
Another component of acid rain is nitric acid, which forms when NO2NO2, also a pollutant, reacts with oxygen and water according to the simplified equation 4NO2(g)+O2(g)+2H2O(l) → 4HNO3(aq)4NO2(g)+O2(g)+2H2O(l) → 4HNO3(aq) The generation of the electricity used in a medium-sized home produces about 19 kgkg of NO2NO2 per year. Part A Assuming that there is adequate O2O2 and H2OH2O, what mass of HNO3HNO3, in kgkg, can form from this amount of NO2NO2 pollutant? Express the mass to two significant figures and include the appropriate units.
Balance these chemical equations. (Use the lowest possible whole number coefficients.) (a) SO2 + O2 → SO3 (b) Fe(OH)2 + O2 + H2O → Fe(OH)3 (c) N2H4 + O2 → H2O2 + N2 (d) NH3 + O2 → NO2 + H2O (e) Sr + H2O → Sr(OH)2 + H2 (f) NH3 + O2 → N2 + H2O

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