Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 1. How many moles of Al are necessary to form 76.2 g of AlBr₃ from this reaction: 2 Al(s) + 3 Br₂(l) → 2 AlBr₃(s) ? ____mol 2. What is the mass in grams of H₂ that can be formed from 48.2 grams of NH₃ in the following reaction? 2 NH₃(g) → 3 H₂(g) + N₂(g) ____g 3. What is the difference between actual yield and theoretical yield? A) Actual yield has to do only with the reactants of a reaction, and theoretical yield has to do only with the products of a reaction. B) Actual yield is how much is actually produced in a reaction (it has to be given or measured), and theoretical yield is a calculation that has to be done. C) Actual yield is how much the reaction produces, and theoretical yield is how much a reaction consumes. D) Actual yield has to do with how much you can actually get out of a reaction, and theoretical yield is how much you can get out of a reaction if you have maximum starting materials. 4. 200.0 mL of a 0.900 M solution of KCl is diluted to 600.0 mL. What is the new…arrow_forward17. Atmospheric sulfur dioxide is the main compound that causes acid rain. It reacts with water and oxygen in the atmosphere to form sulfuric acid, H₂SO4 a. Write a balanced chemical equation for this reaction. b. If 150.0 grams of SO₂ are emitted from a power plant, how much sulfuric acid can theoretically be produced? c. If the actual mass of H₂SO₂ formed is 105.0 g, what is the percent yield of the reaction?arrow_forward48arrow_forward
- 106. A chemist carries out this reaction, beginning with 2.10 grams of NaBr and 3.25 grams of Pb(NO3),: 2 NaBr (aq) + Pb(NO3)2 (aq) > PbBr, (s) + 2 NaNO, (aq) a. Which starting material is the limiting reagent? b. What is the theoretical yield of PbBr, in this reaction? c. If the chemist actually isolates 3.5 grams of PbBr,, what is the percent yield of the reaction?arrow_forwardThe solvent dichloromethane (CH 2Cl 2, molar mass 84.93 g/mol) can be prepared by reaction of methane (CH 4, molar mass 16.04 g/mol) with Cl 2 (molar mass 70.90 g/mol), according to the balanced equation, CH 4 + 2 Cl 2---------->CH 2Cl 2 + 2 HCl. a. If 5.00 g of methane and 15.0 g of Cl 2 are used, how many moles of each reactant are used? b. What is the limiting reactant? c. How many moles of product are formed? d. How many grams of product are formed? e. If 5.6 g of product are formed, what is the percent yield of the reaction?arrow_forwardAluminium metal reacts with sulphuric acid, H2SO4, to yield aluminium sulphate and hydrogen gas. Calculate the mass of aluminium metal needed to produce 13.2 g hydrogen. D.arrow_forward
- Titanium (Ti) is a strong, lightweight metal that is used in the construction of rockets, jet engines, and bicycles. It can be prepared by reacting titanium(IV) chloride with magnesium metal at very high temperatures. The products are titanium metal and magnesium chloride. a. Write a balanced chemical equation for this reaction. b. Assuming that the reaction goes to completion, what is the theoretical yield in kilograms of titanium from a reaction involving 35.5 kg of titanium(IV) chloride and 6.53 kg of magnesium?arrow_forwardIn the combustion of butanol (CH 00), what mass (in g) of butanol must react to produce 55.4 g of product? N.B. Combustion is the reaction of a substance with molecular oxygen (O2) to produce water and carbon dioxide.arrow_forwardHydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction CaF2 + H2SO4 → CaSO4 + 2HF In one process, 6.25 kg of CaF2 is treated with an excess of H2SO4 and yields 2.75 kg of HF. Calculate the percent yield of HF.arrow_forward
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