If 34.7 g of AgNO3 react with 28.6 g of H¿SO, according to this UNBALANCED equation below, what is the mass in grams of Ag¿SO, that could be formed? AgNO3(aq) + H2SO, (aq) → Ag,SO4 (s) + HNO3 (aq)

If 34.7 g of AgNO3 react with 28.6 g of H¿SO, according to this UNBALANCED equation below, what is the mass in grams of Ag¿SO, that could be formed? AgNO3(aq) + H2SO, (aq) → Ag,SO4 (s) + HNO3 (aq)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.27PAE: 4.27 Copper reacts with sulfuric acid according to the following equation: 2H2SO4+CuCuSO4+2H2O+SO2...

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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?
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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).
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
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