2. Balance the following chemical equation:_MgCl2 +Al → _Mg +AIC13a. If the chemical reaction uses 78 grams of Al metal, then how many molesof Mg metal will be produced?b. If the chemical reaction uses 143 grams of MgCl2, then how many molesof AlCl3 will be produced?c. If the chemical reaction uses 47.4 grams of Al metal, then how manymoles of AlCl3 will be produced?d. If the chemical reaction uses 56.2 grams of MgCl2, then how many molesof Mg metal will be produced?e. If the chemical reaction uses 4.2 x 103 grams of Al metal, then how manymoles of MgCl2 will be needed to fully react all of the Al metal?f. If the chemical reaction produces 25.3 grams of Mg metal, then how manymoles of AlCl3 will also be produced?g. If the chemical reaction produces 2.19 x 102 grams of AlCl3, then howmany moles of MgCl2 were needed?h. If the chemical reaction produces 8.33 x 10² grams of AlCl3, then howmany moles of Mg metal were needed?If the chemical reaction produces 119.2 grams of Mg metal, then howmany moles of Al metal were needed?i.

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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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 5.4 kgkg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
Use the following information to answer this question. 2Al) + 3CuCl2(aq)→ 2AICI3(aq) + 3Cu(s) (word equation: aluminum plus three copper(Il) chloride produce two aluminum chloride and three copper) Which of the following best describes what is occurring during this reaction? Select one: O a. Aluminum replaces chlorine in the compound. O b. Aluminum replaces copper in the compound. O c. Copper replaces aluminum in the compound. O d. Chlorine replaces copper in the compound. Smoke Signal.pdf EFiles (1).zip Chap6 SF10 (1).pdf
Potassium chlorate decomposes to potassium chloride and oxygen, as shown in the equation below. 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) Which of the following sentences is a correct expression for a relationship between substances in this reaction? a. One mole of potassium chlorate decomposes into one mole of potassium chloride and one mole of oxygen. b. Two moles of potassium chlorate decompose into two moles of potassium chloride and three moles of oxygen. c. Two liters of potassium chlorate decompose into two liters of potassium chloride and three liters of oxygen. d. Two grams of potassium chlorate decompose into two grams of potassium chloride and three grams of oxygen.
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H5 Cl + C₂2 HOC13 → C14H9 Cl5 + H₂O chlorobenzene chloral DDT In a government lab, 1167 g of chlorobenzene is reacted with 470 g of chloral. a. What mass of DDT is formed, assuming 100% yield? g b. Which reactant is limiting? Which is in excess? is limiting. Mass= is in excess. c. What mass of the excess reactant is left over? g in excess d. If the actual yield of DDT is 285.0 g, what is the percent yield? Percent yield = % Mass=
Glucose (CeH12O6) can be fermented to yield ethanol (C2H5OH) and carbon dioxide (CO2). a. What is the theoretical yield of ethanol (in grams) produced with a 72% yield2 and actual yield of 43.5 g? b. What is the mass of glucose (in grams) in the fermentation reaction? C6H1206 → 2 C2HSOH + 2 cO2 Molar mass of CGH1206 = 180.156 g/mol Molar mass of C2HSOH = 46.07 g/mol Molar mass of CO2 = 44.01 g/mol
the balance chemical equation is P4(s) + 6Cl2(g) -> 4PCl3(g). what is the mass in grams of phosphorus trichloride that can be formed from 150.1 grams of P4 based on the balanced chemical equation?
The thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rockets. In the thermite reaction, iron(III) oxide reacts with elemental aluminum to form aluminum oxide and elemental iron. Write a balanced equation for this reaction. What mass of iron(III) oxide must be used to produce 15.0 g elemental iron? What mass of aluminum oxide will be produced when 15.0 g of iron is produced?
6. Consider the reaction: 2Sb(s) + 312(s) → 2Sbl3(s). Determine the limiting reactant and the theoretical yield when 1.20g of Sb and 2.4g of lz are mixed? What mass of the excess reactant is left when the reaction is complete?
Consider the following reaction for the formation of aluminum sulfate. 2AI(OH) 3 + 3H 2 SO 4 → Al 2 (SO 4) 3+ 6H 2 0 A quantity of 5.07 g Al(OH)3 are mixed with 5.93 g H2SO4. What is the theoretical yield of aluminum sulfate? O 5.56 g O 11.1g O 2.74 g O 6.90 g
[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant. Step 3: Determine the limiting reactant. You have determined complete reaction of 64.7 g aluminum (Al) would give a theoretical yield of 122 g aluminum oxide (Al2O3), whereas complete reaction of 201 g iron (III) oxide (Fe203) would give a theoretical yield of 128 g aluminum oxide (Al203). Which of the following substances is the limiting reactant? A) aluminum (AI) B) iron (III) oxide (Fe2O3) C) aluminum oxide (Al2O3) D) iron (Fe)
Given the following decomposition reaction: 4C3H5O9N3 → O2 + 12CO2 + 10H2O +6N2. a. If 28.40 g H2O were produced, what mass of CO2 will be produced? b. If 110.5 g of C3H5O9N3 were decomposed and the yield of the reaction is 72.3%, determine the theoretical yield and actual yield.
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