Gaseous ethane (CH,CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,O). If 0.0711 g of water is produced from the reaction of 0.30 g of ethane and 0.46 g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.

Gaseous ethane (CH,CH,) reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,O). If 0.0711 g of water is produced from the reaction of 0.30 g of ethane and 0.46 g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 49A

See similar textbooks

Similar questions

In a blast furnace at high temperature, iron(III) oxide in ore reacts with carbon monoxide to produce metallic iron and carbon dioxide. The liquid iron produced is cooled and weighed. The reaction is run repeatedly with the same initial mass of iron(III) oxide, 19.0 g, but differing initial masses of carbon monoxide. The masses of iron obtained arc shown in this graph. (a) Write the balanced chemical equation for this reaction. (b) Calculate the mass of CO required to react completely with 19.0 g iron(III) oxide. (c) Calculate the mass of carbon dioxide produced when the reaction converts 10.0 g iron(III) oxide completely to products. (d) From the graph, determine which reactant is limiting when less than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (e) From the graph, determine which reactant is limiting when more than 10.0 g carbon monoxide is available to react with 19.0 g iron(III) oxide. (f) Calculate the percent yield if 24.0 g iron(III) oxide reacted with 20.0 g carbon monoxide to produce 15.9 g metallic iron. (g) Calculate the minimum mass of additional limiting reactant required to react with all of the excess of nonlimiting reactant from part (f).
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): :math>C5H12(l)+O2(g)CO2(g)+H2O(l) a 20.4-gram sample of pentane is burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
Sulfur dioxide gas reacts with sodium hydroxide to form sodium sulfite and water. The unbalanced chemical equation for this reaction is given below: SO2(g)+NaOH(s)Na2SO3(s)+H2O(l) Assuming you react 38.3 g sulfur dioxide with 32.8 g sodium hydroxide and assuming that the reaction goes to completion, calculate the mass of each product formed.
Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfuric acid. The unbalanced equation is :math>CuO(s)+H2SO4(aq)CuSO4(aq)+H2O(l) 2.49 g of copper(II) oxide is treated with 5.05 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced?
If baking soda (sodium hydrogen carbonate) is heated strongly, the following reaction occurs: :math>2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) lculate the mass of sodium carbonate that will remain if a 1.52-g sample of sodium hydrogen carbonate is heated.
Consider the following reaction: 4NH3(g)4NO(g)+6H2O(g) If a container were to have 10 molecules of O2 and 10 molecules of NH3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?
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?
Small quantities of ammonia gas can be generated in the laboratory by heating an ammonium salt with a strong base. For example, ammonium chloride reacts with sodium hydroxide according to the following balanced equation: :math>NH4Cl(s)+NaOH(s)NH3(g)+NaCl(s)+N2O(g) at mass of ammonia gas is produced if 1.39 g of ammonium chloride reacts completely?
Consider the following balanced chemical equation: A+5B3C+4D a. Equal masses of A and B are reacted. Complete each of the following with either A is the limiting reactant because ; B is the limiting reactant because ____ ; or we cannot determine the limiting reactant because _____ i. If the molar mass of A is greater than the molar mass of B, then ii. If the molar mass of B is greater than the molar mass of A, then b. The products of the reaction are carbon dioxide (C) and water (D). Compound A has a similar molar mass to carbon dioxide. Compound B is a diatomic molecule. Identify compound B, and support your answer. c. Compound A is a hydrocarbon that is 81.7 1% carbon by mass. Determine its empirical and molecular formulas.