7. Са + CaCl2 + Hz When 15.3 g Ca react with 4.5 g of HCI HCI a. Which is the limiting reactant? b. How many formula units of calcium chloride are produced? C. How many liters of hydrogen gas are produced? d. If 1.15 L of hydrogen gas are produced in the lab, what is the percent yield?

7. Са + CaCl2 + Hz When 15.3 g Ca react with 4.5 g of HCI HCI a. Which is the limiting reactant? b. How many formula units of calcium chloride are produced? C. How many liters of hydrogen gas are produced? d. If 1.15 L of hydrogen gas are produced in the lab, what is the percent yield?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 19PS

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Moles within Moles and Molar Mass Part 1: a How many hydrogen and oxygen atoms are present in 1 molecule of H2O? b How many moles of hydrogen and oxygen atoms are present in 1 mol H2O? c What are the masses of hydrogen and oxygen in 1.0 mol H2O? d What is the mass of 1.0 mol H2O? Part 2: Two hypothetical ionic compounds are discovered with the chemical formulas XCl2 and YCl2, where X and Y represent symbols of the imaginary elements. Chemical analysis of the two compounds reveals that 0.25 mol XCl2 has a mass of 100.0 g and 0.50 mol YCl2 has a mass of 125.0 g. a What are the molar masses of XCl2 and YCl2? b If you had 1.0-mol samples of XCl2 and YCl2, how would the number of chloride ions compare? c If you had 1.0-mol samples of XCl2 and YCl2, how would the masses of elements X and Y compare? d What is the mass of chloride ions present in 1.0 mol XCl2 and 1.0 mol YCl2? e What are the molar masses of elements X and Y? f How many moles of X ions and chloride ions would be present in a 200.0-g sample of XCl2? g How many grams of Y ions would be present in a 250.0-g sample of YCl2? h What would be the molar mass of the compound YBr3? Part 3: A minute sample of AlCl3 is analyzed for chlorine. The analysis reveals that there are 12 chloride ions present in the sample. How many aluminum ions must be present in the sample? a What is the total mass of AlCl3 in this sample? b How many moles of AlCl2 are in this sample?
2 NaHCO3 (s) → Na2CO3 (s) + CO2 (g) + H2O (g)1. Calculate the moles of NaHCO3 in 3.00 g of NaHCO3.2. Using your answer to question one, if 1 mole of Na2CO3 is produced for every 2 moles of NaHCO3, how many moles of Na2CO3 would theoretically be produced in the reaction?3. How many grams of Na2CO3 would theoretically be produced in the reaction?4. If the actual mass of Na2CO3 produced is 1.25 g, what is the percent yield of Na2CO3? 5. Calculate the theoretical mass of H2O produced from the decomposition of 3.00 g NaHCO3 using similar calculations as above.
1)How many outer-shell electrons do each of the atoms have? Rn Ga C Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+Cl2(g) A sample of 42.1 g MnO2 is added to a solution containing 49.9 g HCl. What is the limiting reactant? MnO2 or HCl 2) What is the theoretical yield of Cl2? theoretical yield: 3) If the yield of the reaction is 80.5%, what is the actual yield of chlorine? actual yield: 4) For the chemical reaction shown, 2H2O2(l)+N2H4(l)⟶4H2O(g)+N2(g) determine how many grams of N2 are produced from the reaction of 8.06 g of H2O2 and 5.39 g of N2H4. N2 produced:
Use the following information to answer questions 3.2, 3.3, and 3.4.Calcium phosphide (Ca3P2) and water react to form calciumhydroxide and phosphine (PH3). In a particular experiment,225.0 g Ca3P2 and 125.0 g water are combined.Ca3P2(s) + H2O(l) Ca(OH)2(aq) + PH3(g)(Don’t forget to balance the equation.) 3.2How much PH3 can be produced?(a) 350.0 g (b) 235.0 g (c) 78.59 g (d) 83.96 g (e) 41.98 g3.3How much Ca(OH)2 can be produced?(a) 91.51 g (b) 274.5 g (c) 513.8 g (d) 85.63 g (e) 257.0 g3.4How much of the excess reactant remains when the reaction iscomplete?(a) 14.37 g (b) 235.0 g (c) 78.56 g (d) 83.96 g (e) 41.98 g
2Fe2O3 + 3C → 3CO2 + 4Fe C. How many grams of Fe are produced from 1.88g of C?
When 8.00 g of Aluminum is allowed to react with 35.0 g of chlorine gas to produce aluminum chloride, which reagent is used up completely and how much product is formed? 2Al+3CCl2=2AlCl3
If 4.0 mol of NO and 4.0 mol of O2 are combined, how many moles of NO2 are produced? 2NO + O2 -> 2NO2
Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2(s) + 2H2O(l) → Sr(OH)2(s) + 2H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 2.81 g of SrH2 and 2.34 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH2?(b) How many moles of H2 can be produced from the given mass of H2O? (c) Which is the limiting reactant? (d) How many grams of H2 can be produced?
Ethanol, C2H5OH, has a density of 0.785 g/mL and a molar mass of 46.07 g/mol. How many moles of ethanol are present in 1.00 L of pure ethanol (A) 17.0 moles (B) 21.7 moles (C) 27.7 moles (D) 2.77 moles
91. Ammonia reacts with O₂ to form either NO(g) or NO₂(g) according to the following UNBALANCED equations: NH₃(g) + O₂(g) → NO(g) + H₂O(g) NH₃(g) + O₂(g) → NO₂(g) + H₂O(g) In one experiment 6.00 moles of NH₃(g) and 15.00 moles of O₂(g) were placed in a closed flask and allowed to react. After the reaction was complete, 6.75 moles of O₂(g) remained and all of the NH₃(g) had reacted. Calculate the number of moles of NO(g) formed in the reaction mixture.
6. Consider the reaction of solid PbO and gaseous NH₃ to form solid Pb, nitrogen gas, and water vapor. a. The balanced chemical equation is 3 PbO(s) + 2 NH₃(g) → 3 Pb(s) + N₂(g) + 3 H₂O(g). How many moles of NH₃ are required to produce 185.6 grams of Pb based on the balanced chemical equation? b. How many grams of N₂ will be produced from 0.447 moles of PbO balanced chemical equation? c. How many grams of NH₃ will be required to react with 32.7 grams of PbO based on the balanced chemical equation? (Part a shown in picture)
How many moles of calcium hydroxide are made from 5.3 moles of water? CaC2 + 2H20 ---> C2H2 + Ca(OH)2

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