5 Gaseous methane (CH)reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,O). If 0.248 g of water isproduced from the reaction of 0.16 g of methane and 0.86 g of oxygen gas, calculate the percent yield of water.Be sure your answer has the correct number of significant digits in it.

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Answered: e percent yield of water.

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e percent yield of water.

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 49A

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Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

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Gaseous methane (CH)
reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,O). If 0.248 g of water is
produced from the reaction of 0.16 g of methane and 0.86 g of oxygen gas, calculate the percent yield of water.
Be sure your answer has the correct number of significant digits in it.

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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).
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