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Problem 46c
For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2( g) → TiF4(s) c. 0.233 g Ti, 0.288 g F2
Problem 47
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
Problem 48
Elemental phosphorus reacts with chlorine gas according to the equation: P4(s) + 6 Cl2( g) → 4 PCl3(l) A reaction mixture initially contains 45.69 g P4 and 131.3 g Cl2. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?
- Lead ions can be precipitated from solution with KCl according to the reaction: Pb2+ (aq) + 2 KCl(aq) → PbCl2(s) + 2 K+ (aq). When 28.5 g KCl is added to a solution containing 25.7 g Pb2+, a PbCl2 precipitate forms. The precipitate is filtered, dried, and found to have a mass of 29.4 g. Determine the percent yield for the reaction. Determine the theoretical yield of PbCl2. Determine the limiting reactant.
Problem 49
Problem 50
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O2(g) → 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O2, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
Problem 51
Urea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2 NH3(aq) + CO2(aq) → CH4N2O(aq) + H2O(l) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.
- Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the limiting reactant and the theoretical yield.
Problem 52
Problem 52c
Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the percent yield for the reaction.
Problem 53a,b
Calculate the molarity of each solution.
a. 3.25 mol of LiCl in 2.78 L solution
b. 28.33 g C6H12O6 in 1.28 L of solution
Problem 53c
Calculate the molarity of each solution.
c. 32.4 mg NaCl in 122.4 mL of solution
Problem 54
Calculate the molarity of each solution. a. 0.38 mol of LiNO3 in 6.14 L of solution b. 72.8 g C2H6O in 2.34 L of solution c. 12.87 mg KI in 112.4 mL of solution
Problem 55
What is the molarity of NO3– in each solution? a. 0.150 M KNO3 b. 0.150 M Ca(NO3)2 c. 0.150 M Al(NO3)3
Problem 56a
what is the molarity of Cl- in each solution? a. 0.200 M NaCl
Problem 56b
What is the molarity of Cl- in each solution? b. 0.150 M SrCl2
Problem 56c
what is the molarity of Cl- in each solution? c. 0.100 M AlCl3
Problem 57a
How many moles of KCl are contained in each solution? a. 0.556 L of a 2.3 M KCl solution
Problem 57b
How many moles of KCl are contained in each solution? b. 1.8 L of a 0.85 M KCl solution
Problem 57c
How many moles of KCl are contained in each solution? c. 114 mL of a 1.85 M KCl solution
Problem 58a
What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? a. 0.45 mol ethanol
Problem 58b
What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? b. 1.22 mol ethanol
Problem 58c
What volume of 0.200 M ethanol solution contains each amount in moles of ethanol? c. 1.2⨉10-2 mol ethanol
Problem 59
A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3 (in g) is needed?
Problem 60
A chemist wants to make 5.5 L of a 0.300 M CaCl2 solution. What mass of CaCl2 (in g) should the chemist use?
Problem 61
If 123 mL of a 1.1 M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted solution?
Problem 62
If 3.5 L of a 4.8 M SrCl2 solution is diluted to 45 L, what is the molarity of the diluted solution?
Problem 63
To what volume should you dilute 50.0 mL of a 12 M stock HNO3 solution to obtain a 0.100 M HNO3 solution?
- Consider the precipitation reaction: 2 Na3PO4(aq) + 3 CuCl2(aq) → Cu3(PO4)2(s) + 6 NaCl(aq). What volume of 0.175 M Na3PO4 solution is necessary to completely react with 95.4 mL of 0.102 M CuCl2?
Problem 65
Problem 66
Consider the reaction: Li2S(aq) + Co(NO3)2(aq) → 2 LiNO3(aq) + CoS(s) What volume of 0.150 M Li2S solution is required to completely react with 125 mL of 0.150 M Co(NO3)2?
Problem 67
What is the minimum amount of 6.0 M H2SO4 necessary to produce 25.0 g of H2(g) according to the reaction between aluminum and sulfuric acid? 2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)
Problem 68
What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 275 mL. Zn(s) + CuCl2(aq) → ZnCl2(aq) + Cu(s)