Iron (III) oxide reacts with carbon monoxide to produce iron andcarbon dioxide.Fe2O3 (s) + 3CO(g) →2Fe(s) + 3CO2(g)tabps lockescaltAcontrol optionF1Z5,389@2F2WSJUL27XHcommandㅁㅁ#3F3ED440CDOO000Part AWhat is the percent yield of iron if the reaction of 64.0 g of iron (III) oxide produces 14.8 g of iron?Express your answer to three significant figures.V| ΑΣΦRF4Fe=SubmitPart BFCO₂ =What is the percent yield of carbon dioxide if the reaction of 73.6 g of carbon monoxide produces 88.4 g of carbon dioxide?Express your answer to three significant figures.ΠΕ ΑΣΦSubmit15%5CRequest AnswerVRequest AnswerF5TGMacBook AirBF6Y&7HtvF7UN??*8%▶IIF8LMA9KOF9OH0LcommandXF10PWF11alt{option[

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Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe₂O3(s) +3CO(g) →2Fe(s) + 3CO2 (8) Y Y Part A What is the percent yield of iron if the reaction of 64.0 g of iron(III) oxide produces 14.8 g of iron? Express your answer to three significant figures. ΠΕ| ΑΣΦ Fe= Submit Part B Request Answer CO₂ = What is the percent yield of carbon dioxide if the reaction of 73.6 g of carbon monoxide produces 88.4 g of carbon dioxic Express your ansv significant figures. ΠΟΠ ΑΣΦ 3 ? d C % ? %

Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Fe₂O3(s) +3CO(g) →2Fe(s) + 3CO2 (8) Y Y Part A What is the percent yield of iron if the reaction of 64.0 g of iron(III) oxide produces 14.8 g of iron? Express your answer to three significant figures. ΠΕ| ΑΣΦ Fe= Submit Part B Request Answer CO₂ = What is the percent yield of carbon dioxide if the reaction of 73.6 g of carbon monoxide produces 88.4 g of carbon dioxic Express your ansv significant figures. ΠΟΠ ΑΣΦ 3 ? d C % ? %

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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The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
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?
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)
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation? lf 2.50 moles of A2 are reacted with excess AB, what amount (moles) of product will form? If the mass of AB is 30.0 u and the mass of A2 are 40.0 u, what is the mass of the product? If 15.0 g of AB is reacted, what mass of A2 is required to react with all of the AB, and what mass of product is formed?
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 an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reac- tion has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
For the chemical reaction C3H8O2+4O23CO2+4H2O how many product molecules are formed when nine C3H8O2 molecules react?
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