Consider the following reaction: C4H9OH + NaBr + H2SO4 C4H9B +NaHSO4 + H20 If 30.0 g of C4H9OH reacts with 44.8 g of NaBr and 65.4 g of H2SO4 according to the balanced equa a. Use C4H9Br to determine the limiting reagent (show all calculations). b. What mass of the excess reagents remain unreacted? C. If 34.2 g of C4H9BR was produced, what is the percentage yield of the reaction?

Consider the following reaction: C4H9OH + NaBr + H2SO4 C4H9B +NaHSO4 + H20 If 30.0 g of C4H9OH reacts with 44.8 g of NaBr and 65.4 g of H2SO4 according to the balanced equa a. Use C4H9Br to determine the limiting reagent (show all calculations). b. What mass of the excess reagents remain unreacted? C. If 34.2 g of C4H9BR was produced, what is the percentage yield of the reaction?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 9RQ: Consider the following mixture of SO2(g) and O2(g). If SO2(g) and O2(g) react to form SO3(g), draw a...

See similar textbooks

Similar questions

DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
Citric acid (C6H8O7) is made by fermentation of sugarssuch as sucrose (C12H22O11) in air. Oxygen is consumedand water generated as a by-product. (a) Write a balanced equation for the overall reaction thatoccurs in the manufacture of citric acid from sucrose. (b) What mass of citric acid is made from 15.0 kg sucrose?
(a) Butane gas, C4H10, can burn completely in air [use O2(g) as the other reactant] to give carbon dioxide gas and water vapor. Write a balanced equation for this combustion reaction. (b) Write a balanced chemical equation for the complete combustion of C3H7BO3, a gasoline additive. The products of combustion are CO2(g), H2O(g), and B2O3(s).
How many moles of beryllium (Be) are needed to completely react with 10.0 moles of N2 in the synthesis of the compound Be3N2?
Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen. CO(g) + 2 H2(g) CH3OH(l) What mass of hydrogen is required to produce 1.0 L of CH3OH (d = 0.791 g/mL) if this reaction has a 74% yield under certain conditions?
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
Consider the following mixture of SO2(g) and O2(g). If SO2(g) and O2(g) react to form SO3(g), draw a representation of the product mixture assuming the reaction goes to completion. What is the limiting reactant in the reaction? If 96.0 g of SO2 react with 32.0 g O2, what mass o f product will form?