5) Isopentyl acetate (aka banana oil) can be prepared by an esterification reaction using acetic acid and isopentyl alcohol. The balanced reaction is shown below. If a student reacts 5.50 mL of acetic acid with 2.35 mL of isopentyl alcohol and obtains 3.25 mL of isopentyl acetate as the product, what was the percent yield of the reaction? H* + H20 HO, HO, acetic acid isopentyl alcohol isopentyl acetate bp 142 °C bp 118 °C bp 129 °C MW 60.0 MW 88.2 MW 130.2 d. 1.05 g/mL d. 0.810 g/mL d. 0.867 g/mL

5) Isopentyl acetate (aka banana oil) can be prepared by an esterification reaction using acetic acid and isopentyl alcohol. The balanced reaction is shown below. If a student reacts 5.50 mL of acetic acid with 2.35 mL of isopentyl alcohol and obtains 3.25 mL of isopentyl acetate as the product, what was the percent yield of the reaction? H* + H20 HO, HO, acetic acid isopentyl alcohol isopentyl acetate bp 142 °C bp 118 °C bp 129 °C MW 60.0 MW 88.2 MW 130.2 d. 1.05 g/mL d. 0.810 g/mL d. 0.867 g/mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 7RQ: Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation?...

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4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
4.70 The particulate scale drawing shown depicts the products of a reaction between H2 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.
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.
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.
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?
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
4-93 Ammonia is prepared industrially by the reaction of nitrogen and hydrogen according to the following equation: If 29.7 kg of N2 is added to 3.31 kg of H2, (a) Which reactant is the limiting reagent? (b) How many grams of the other reactant are left over? (c) How many grams of NH3 are formed if the reaction goes to completion?
Methanol, CH3OH, is used in racing cars because it is a clean-burning fuel. It can be made by this reaction: CO(g)+2H2(g)CH3OH(l) What is the percentage yield if 5.0103gH2 reacts with excess CO to form 3.5104gCH3OH ?
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.
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.
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
4.69 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. 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.