Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H20. If 0.817g of carbon dioxide is produced from the reaction of 0.48g of methane and 3.6g of oxygen gas, calculate the percent yield of carbon dioxide

Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H20. If 0.817g of carbon dioxide is produced from the reaction of 0.48g of methane and 3.6g of oxygen gas, calculate the percent yield of carbon dioxide

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 154AE: Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces...

See similar textbooks

Similar questions

Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
Calculate the amounts of reactants needed in a chemical reaction to produce a specified amount of product.
Quicklime, CaO, is formed when calcium hydroxide is heated. Ca(OH)2(s) → CaO(s) + H2O(ℓ) The theoretical yield is 65.5 g but only 36.7 g quicklime I is produced. Calculate the percent yield.
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
Billions of pounds of urea, CO(NH2)2, are produced annually for use as a fertilizer. The principal reaction employed is: 2NH3+CO2CO(NH2)2+H2O By assuming unlimited amounts of CO2, how many moles of urea can be produced from each of the following amounts of NH3? a.2molNH3b.0.45molNH3c.10gNH3d.2.0kgNH3
The sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)
Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, hcpLcnc reacts with oxygen to produce carbon dioxide and water. What is the mole ratio that would enable you to calculate the number of moles of oxygen needed to react exactly with a given number of moles of heptene? What mole ratios would you use to calculate how many moles of each product form from a given number of moles of heptene?
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.
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.
The iron oxide Fe2O3 reacts with carbon monoxide (CO)to give iron and carbon dioxide: Fe2O3+3CO2Fe+3CO2 The reaction of 433.2 g Fe2O3 with excess CO yields254.3 g iron. Calculate the theoretical yield of iron(assuming complete reaction) and its percentage yield.