An "ideal" fuel'air mixture in which both the fuel and the oxygen in the air are completely consumed is called the "stoichiometric" mixture. The stoichiometric mixture is usually specified as the ratio of the mass of air to the mass of a particular fuel. For example, if a fuel (for example, natural gas, CH4) required 17.2 kg of air to precisely burn 1 kg of the fuel (that is, all the fuel burned and there was no oxygen left in the air afterwards) then the stoichiometric ratio for that fuel would be 17.2: 1. Calculate the partial pressures of the natural gas and oxygen in the mixture based on the stoichiometric ratio given above at 293.15 K. The volume of the internal combustion engine is considered to be 2.500 L. The mass of the fuel is 160.0 g. Mass fraction of oxygen in air is 23.1%. Molar mass of natural gas is 16.043 g/mol. P natural gas = atm Poxygen=[ atm

An "ideal" fuel'air mixture in which both the fuel and the oxygen in the air are completely consumed is called the "stoichiometric" mixture. The stoichiometric mixture is usually specified as the ratio of the mass of air to the mass of a particular fuel. For example, if a fuel (for example, natural gas, CH4) required 17.2 kg of air to precisely burn 1 kg of the fuel (that is, all the fuel burned and there was no oxygen left in the air afterwards) then the stoichiometric ratio for that fuel would be 17.2: 1. Calculate the partial pressures of the natural gas and oxygen in the mixture based on the stoichiometric ratio given above at 293.15 K. The volume of the internal combustion engine is considered to be 2.500 L. The mass of the fuel is 160.0 g. Mass fraction of oxygen in air is 23.1%. Molar mass of natural gas is 16.043 g/mol. P natural gas = atm Poxygen=[ atm

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...

See similar textbooks

Similar questions

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 7.8kg of octane burned.
The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H₁206+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" 3.00 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. 0 X
A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 45.0 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? _ g [Number in standard notation; round your answer to one decimal place] The following molar masses may or may not be needed, but are provided to save you time: barium sulfate = 233 g/mol sulfuric acid = 98.0 g/mol
Consider the reaction. heat 2 Al(s) + Fe,03(s) Al,0;(s) + 2 Fe(l) If 11.5 kg Al reacts with an excess of Fe,O3, how many kilograms of Al,O, will be produced? mass of Al,0, produced:
Consider the reaction. heat 2 Al(s) + Fe,0,(s) Al,03(s) + 2 Fe(1) If 11.5 kg Al reacts with an excess of Fe,O2, how many kilograms of Al,0, will be produced? mass of Al,0, produced: kg
magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. When 10.1 g of Mg reacts with 10.5 g of O2, 11.9 g of MgO are collected. What is the balanced equation for this reaction, including all states of matter?
The coefficients in a balanced chemical equation provide the mole-to- mole stoichiometry among the reactants and products. The molar mass (in g/mol) can be used as the conversion factor between moles and the mass of a substance. Thus, the balanced equation and molar masses can be used in conjunction with one another to calculate the masses involved in a reaction. Complete combustion of methane When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH₂(g) + O₂(g) →CO₂(g) + H₂O(g) This type of reaction is referred to as a complete combustion reaction. Review Constants Perio Part A What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H₂O, respectively. Express your answer as four integers, separated by commas (e.g., 1,2,3,4).
Hydrogen sulfide, H2S, is produced during decomposition of organic matter. When 0.4190 mol H2S burns to produce SO2 (9) and H20(g), -217.0 kJ of heat is released. What is this heat in kilocalories? Heat = kcal
A sample of 49.0 g of tetraphosphorous decoxide (P,O10) reacts with 49.0 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,010 + 6 H,O → 4H,PO, Determine the limiting reactant for the reaction. H,PO, O H,0 O P,O10 Calculate the mass of H, PO, produced in the reaction. mass of H, PO4: Calculate the percent yield of H, PO, if 37.5 g of H, PO, is isolated after carrying out the reaction. percent yield:
In the "Methodé Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is )) C6H1206(aq) → 2C2H50H(aq) + 2C02(g) Fermentation of 750. mL of grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume of 825. mL until 12.5% by volume is ethanol (C,H;OH). Assuming that the Co, is insoluble in H,0 (actually a wrong assumption), what would be the pressure of CO, inside the wine bottle at 25°C? (The density of ethanol is 0.79 g/cm3)
What is the easiest process to get to the result?
Soda ash (sodium carbonate) is widely used in the manufacture of glass. Prior to the environmental movement much of it was produced by the following reaction. CaCO3 + 2 NaCl → Na2CO3 + CaCl2 Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem. As a result of the environmental movement, all of these plants closed. Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react. Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced. How many grams of useless calcium chloride (110.98 g/mol) will be produced? You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)