CHAPTER 3. CH7 PROBLEM SOLVING CLASS R.D. A. BOLINAS. http:// chempsclass.wordpress.com. 3.10 Calculate the molar mass of each of the following: (a) N 2 O 4 ( b ) C 8 H 10 ( c ) MgSO 4 ⦁7H 2 O ( d ) Ca(C 2 H 3 O 2 ) 2. a) N 2 O 4 = 2(14.01) + 4(16.00) = 92.02 g/ mol
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CH7 PROBLEM SOLVING CLASS
R.D. A. BOLINAS
3.14 Calculate each of the following quantities:(a) Total number of ions in 38.1 g of SrF2(b) Mass in kilograms of 3.58 mol of CuCl2 2H2O(c) Mass in milligrams of 2.88 x1022formula units of Bi(NO3)3⦁ 5H2O
3.23 Hemoglobin, a protein in red blood cells, carries O2 from the lungs to the body’s cells. Iron (as ferrous ion, Fe2+) makes up 0.33 mass % of hemoglobin. If the molar mass of hemoglobin is 6.8x 104 g/mol, how many Fe2+ions are in one molecule?
3.26 What is the empirical formula and empirical formula massfor each of the following compounds?(a) C4H8(b) C3H6O3(c) P4O10(d) Ga2(SO4)3(e) Al2Br6
3.32 A 0.370-mol sample of a metal oxide (M mass2O3) weighs 55.4 g.(a) How many moles of O are in the sample?(b) How many grams of M are in the sample?(c) What element is represented by the symbol M?
3.38Write balanced equations for each of the following by massinserting the correct coefficients in the blanks:(a) __Cu(NO3)2(aq) + __KOH(aq) ⟶__Cu(OH)2(s) + __KNO3(aq)(b) __BCl3(g) + __H2O(l) ⟶__H3BO3(s) + __HCl(g)(c) __CaSiO3(s) + __HF(g) ⟶__SiF4(g) + __CaF2(s) + __H2O(l)(d) __(CN)2(g) __H2O(l)⟶ __H2C2O4(aq) __NH3(g)
Cu(OH)2(s) + 2 KNO3(aq)
3.41 The molecular scene at right massrepresents a mixture of A2 (blue) and B2(green) before they react to form AB3.(a) What is the limiting reactant?(b) How many molecules of product can form?
would be required. Since you have only 6 B2 molecules, B2is the limiting reagent.
b) 6 B2 molecules x (2 AB3 / 3 B2) = 4 AB3 molecules
3.51 Calculate the maximum numbers of moles and grams of massH2S that can form when 158 g of aluminum sulfide reacts with 131 g of water:Al2S3 + H2O ⟶ Al(OH)3 + H2S [unbalanced]What mass of the excess reactant remains?
3.66 Six different aqueous solutions (with solvent massmolecules omitted for clarity) are represented in the beakers below, and their total volumes are noted.
A B C
D E F
(a mass) Which solution has the highest molarity? (b) Which solutions have the same molarity? (c) If you mix solutions A and C, does the resulting solution have a higher, a lower, or the same molarity as solution B?
A B C
D E F
(d) After 50. mL of water is added to solution massD, is its molarity higher, lower, or the same as that of solution F after 75 mL of water is added to it?
A B C
D E F
A B C
D E F
3.69 Solution E has the equivalent of 4 particles in a volume of 50 Calculate each of the following quantities:(a) Volume in milliliters of 2.26 M potassium hydroxide thatcontains 8.42 g of solute(b) Number of Cu2 ions in 52 L of 2.3 M copper(II) chloride(c) Molarity of 275 mL of solution containing 135 mmol of glucose
H Solution E has the equivalent of 4 particles in a volume of 50
3.83 One of the compounds used to increase the octane rating of gasoline is toluene (right).Suppose 20.0 mL of toluene(d = 0.867 g/mL) is consumedwhen a sample of gasoline burnsin air. (a) How many grams ofoxygen are needed for complete combustion of the toluene?(b) How many total moles of gaseous products form? (c) How many molecules of water vapor form?