The balanced equation for the combustion of butane, CAH10, is shown below. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 CH10(g) + 13 02(g) --> 8 CO,(g) + 10 H20(1) 58.124 32 44.011 18.016 How many liters of oxygen gas will be required to burn 2.00 L of butane in this reaction?

The balanced equation for the combustion of butane, CAH10, is shown below. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 CH10(g) + 13 02(g) --> 8 CO,(g) + 10 H20(1) 58.124 32 44.011 18.016 How many liters of oxygen gas will be required to burn 2.00 L of butane in this reaction?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 165MP

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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.
62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
How many moles of O2 are needed to burn 1.45 mol of C8H18? Express the amount in moles to three significant digits. The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g) Relevant volumetric equivalencies 1 gal = 3.785 L 1 L = 1000 mL
The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: 12 C6H12O6 +602-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.8 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³.
The so called hydrogen economy is based on hydrogen produced from water using solar energy. The gas may be burned as a fuel: 2H2 (g) + O2 (g) ---> 2H2O (l) A primary advanatge of hydrogen as a fuel is that it is nonpolluting. A major disadvantege is that it is a gas and therefore is harder to store than liquids or solids. Calculate the volume of hydrogen gas at 25oC and 1.00 atm required to produce an amount of energy equivalent to that produced by the combustion of a gallon of octane (C8H18). The density of cotane is 2.66 kg/gal and its standard entalpy of formation is -249.9 kj/mol.
The human body burns glucose C6H12O6 for energy according to this chemical reaction:→+C6H12O66O2+6CO26H2O. The products of the reaction are carbon dioxide CO2 and water H2O. Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mLof air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 3.0kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 2.00kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0/kgm3
The human body burns glucose (C6H12O6) for energy according to this chemical reaction: C6H12O6+6O2→ 6CO2+6H2O The products of the reaction are carbon dioxide CO2 and water H2O Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500.mL of air, which is typically enriched to 4% CO2 and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 0.50kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO2 is 2.0 kg/m^3 .
Solid ammonium chloride, NH,Cl, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH; (g)+HCl(g) NH, CI(s) A 6.75 g sample of NH, gas and a 6.75 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C. Identify the limiting reagent. NH,C1 HCl NH, How many grams of NH, Cl will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH,Cl produced by the reaction. P = atm
One of the principal components of gasoline is octane 10 (C_8H_{18}; MW= 114.23 g/mol). What mass of oxygen gas (O_2; 32.00 g/mol) from the air is consumed in the combustion of 702 g of octane? The unbalanced chemical equation is shown below. * C3H18(1) + 02(g) → CO2(g)+ H20(9)
9:38 نقطتان )2( Q1. The volume of air(N2 and 02) needed for complete combustion of 1 kg of propane * -:(C3H8 ) is 21 O 15.9 O 18.8 O 23.8 O ع غ ف ق ث ص ض ي س ش 123 مسافة اذهب J.
Solid ammonium chloride, NH,CI, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH, (g) + HCI(g) – NH,CI(s) A 3.43 g sample of NH, gas and a 3.43 g sample of HCI gas are mixed in a 1.50 L flask at 25 "C. Identify the limiting reagent. ONH,CI HCI NH, How many grams of NH, CI will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH Cl produced by the reaction.
Reso- Solid ammonium chloride, NH, CI, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH, (g)+HCI(g) NH,CI(s) A 3.12 g sample of NH, gas and a 3.12 g sample of HCI gas are mixed in a 0.50 L flask at 25 °C. Identify the limiting reagent. О НС NH,CI NH, How many grams of NH,CI will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH, CI produced by the reaction. P = atm O O O

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