Be sure to answer all parts.The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°Cand is used in welding metals:2Al + FezO3 → Al,03 +2FeIn one process, 133 g of Al are reacted with 601 g of Fe,O3. Calculate the mass (in grams) of Al,O3formed, and determine the amount of excess reagent left at the end of the reaction.mass of Al,0, formed:amount of excess reagent left:

Answered: Be sure to answer all parts. The…

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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Aspirin (C9H8O4) may be synthesized by mixing salicylic acid (C7H6O3) with excess acetic anhydride (C4H6O3). When 2.0 g of salicylic acid is mixed with excess acetic anhydride, 1.7 g of aspirin is collected. What is the percent yield of this reaction? The balanced equation is C7H6O3 + C4H6O3  C9H8O4 + C2H4O2 A.98 % B.85 % C.77 % D.65 % E.55 %
Ammonia gas can be prepared by the reaction CaO(s) + 2NH4Cl(s) → 2 NH3(g) + H₂O(g) + CaCl₂ (s) In an experiment, 33.0 g of ammonia gas, NH3, is produced when it was predicted that 43.2 g NH3 would form. What is the theoretical yield of NH3 ? theoretical yield: What is the actual yield of NH3 ? actual yield: What is the percent yield of NH3 ? percent yield: 6.0 g 0.0 g %
The formation of potassium chlorate, KClO3, can be represented by the equation (unbalanced): K (s) + Cl2 (g) + O2 (g) = KClO3 (s) The molar masses are; K = 39.1 g/mol; Cl2 = 70.9 g/mol; O2 = 32.0 g/mol If we reacted 100.0 grams of each reagent, which would be the limiting reagent for the reaction? Group of answer choices Cl2 K O2
39.06 g C6H6) + (120.00 g O2) ------------> (132.03 g CO2) + (x g H2O) Assuming that both reactants are completely used up, calculate the numerical value of x. Place your answer in the box
Complete combustion of 4.5892 a particular compound that contains only carbon, hydrogen and oxygen produces 10.4324 g of CO2 and 4.2705 g of H2O. The empirical formula of the compound is given by C H O (indicate "1" if there is only one atom of a given type in the empirical formula.) The molar mass of the compound is found to be 116.16 g/mol in a different experiment. What is the molecular formula of the compound? C H O
Consider the reaction: N2(g) + 202(g) → 2NO2(g) 0.250 mol of N2(g) is reacted with 0.300 mol of O2(g). Calculate the amount of excess reagent in moles remains assuming complete reaction. [Hint: lIdentify the excess reagent first.] Select one: a. 0.150 mol of excess reagent remains. b. 0.200 mol of excess reagent remains. C. 0.050 mol of excess reagent remains. d. 0.100 mol of excess reagent remains.
Write a balanced chemical equation based on the following description: butane gas reacts with oxygen gas to produce carbon dioxide gas and water vapor C4H10(g)+O2(g)_
Consider the following chemical equation: NH4NO3 (s) → N2O (g) + H2O (g) What would be the coefficients in front of each reactant and product in the balanced equation? If there would be no coefficient in front of a given compound in the balanced equation, just write type '1' NH4NO3 =? N2O =? H2O =?
magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. When 10.1 g of Mg reacts with 10.5 g of O2, 11.9 g of MgO are collected. What is the balanced equation for this reaction, including all states of matter?
Acrylonitrile is an important building block for synthetic fibers and plastics. Over 2 billion pounds of acrylonitrile are produced in the United States each year. The compound is synthesized from propene in the following reaction:2C3H6 + 2NH3 + 3O2 → 2C3H3N + 6H2OWhat mass of acrylonitrile can be prepared from 150.0 kg of propene, 600.0 kg of ammonia, and 100.0 kg of oxygen?
The coefficients in a balanced chemical equation provide the mole-to- mole stoichiometry among the reactants and products. The molar mass (in g/mol) can be used as the conversion factor between moles and the mass of a substance. Thus, the balanced equation and molar masses can be used in conjunction with one another to calculate the masses involved in a reaction. Complete combustion of methane When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH₂(g) + O₂(g) →CO₂(g) + H₂O(g) This type of reaction is referred to as a complete combustion reaction. Review Constants Perio Part A What coefficients are needed to balance the equation for the complete combustion of methane? Enter the coefficients in the order CH4, O2, CO2, and H₂O, respectively. Express your answer as four integers, separated by commas (e.g., 1,2,3,4).
Honors Chemistry Chapter 9 Name/Date 3. Gold is very valuable because it does not oxidize easily. It can be oxidized by reacting it with nitric acid as shown below: Au(s) + 4H'(aq) + NO: (aq) → NO(g) + 2H:0(g) + Au³ (aq) 3a. If 30 grams of gold react with 3.4 grams of nitrate ion, which reactant is limiting?. 3b. What is the theoretical yield?. 4. Lead (II) nitrate reacts with sodium chloride according to the equation below: Pb(NO.): + NaCl → PbCla + NANO. 4a. If 8.3 grams of lead (II) nitrate react with 5 grams of sodium chloride, which material would be the limiting reactant? 4b. What is the theoretical yield?

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