<p>EXAM 1 – Form B CHEM 101: Sections 565-576 Dr. M. Shatruk FALL 2005</p><p>1. Stainless steel for marine applications contains chromium and molybdenum – metals which make it highly resistant to corrosion caused by seawater. If the steel is 17% Cr by mass, what is the amount of Cr in grams contained in 955 g of steel? [6 pts]</p><p>(A) 475 g (B) 126 g (C) 162 g (D) 793 g</p><p>2. Determine the percent composition of sodium in Na2SO3: [7 pts]</p><p>(A) 36.5% (B) 38.1% (C) 25.4% (D) 18.8%</p><p>3. How much potassium chloride is produced from the reaction of 2.00 g of K and 3.00 g of Cl2? [8 pts]</p><p>2K + Cl2  2KCl</p><p>(A) 3.15 g (B) 1.90 g (C) 3.81 g (D) 6.31 g</p><p>4. 10.2 g of chromium (Cr) reacts with excess Cl2 to produce 23.9 g of chromium(III) chloride, CrCl3. What is the percent yield of CrCl3? (Don’t forget to balance the equation.) [9 pts]</p><p>(A) 115% (B) 38.5% (C) 90.3% (D) 76.9%</p><p>Page B-1 EXAM 1 – Form B CHEM 101: Sections 565-576 Dr. M. Shatruk FALL 2005</p><p>5. An aqueous solution of KBr contains 114 g of KBr and the concentration of potassium bromide is 6.00%. What is the total mass of the solution? [6 pts]</p><p>(A) 190 g (B) 1900 g (C) 1784 g (D) 160 g</p><p>6. 700 mL of water is added to 100 mL of 1.60 M solution of KOH. What is the molarity of the resulting solution? [6 pts]</p><p>(A) 0.200 M (B) 0.458 M (C) 0.229 M (D) 0.400 M</p><p>7. What volume of 1.60 M solution of LiOH is needed to react with 300 mL of 0.800 M solution of HNO3 according to the equation: [9 pts]</p><p>LiOH + HNO3  LiNO3 + H2O</p><p>(A) 300 mL (B) 250 mL (C) 200 mL (D) 150 mL</p><p>Page B-2 EXAM 1 – Form B CHEM 101: Sections 565-576 Dr. M. Shatruk FALL 2005 Your Name: ______Section #: ______</p><p>8. Express the following numbers in standard exponential form (scientific notation): [5 pts]</p><p>(a) 0.007833 (b) 1 234 000 (c) 34 675</p><p>9. An atom contains 29 electrons and 36 neutrons. Determine: [6 pts]</p><p>(a) the atomic number of the element</p><p>(b) the name of the element</p><p>(c) the number of protons</p><p>(d) the mass of the atom in a.m.u. (calculate the mass without looking at the periodic chart)</p><p>10. Write formulas for the following ionic compounds: [7 pts]</p><p>(a) calcium sulfate</p><p>(b) iron(III) carbonate</p><p>(c) ammonium bromide</p><p>11. A compound contains 56.3% of phosphorus and 43.7% of oxygen. Its molecular weight is 219.9 a.m.u. Derive its molecular formula. [9 pts]</p><p>Page B-3 EXAM 1 – Form B CHEM 101: Sections 565-576 Dr. M. Shatruk FALL 2005</p><p>12. Balance the following equations: [7 pts]</p><p>(a) ZnS + O2  ZnO + SO2</p><p>(b) BiCl3 + H2O  BiOCl + HCl</p><p>13. Classify each of the following substances as acid, base, or salt: [6 pts]</p><p>(a) KOH</p><p>(b) NH4Br</p><p>(c) H2SO4</p><p>(d) Cu(NO3)2</p><p>14. Write the total and net ionic equations for following reactions: [9 pts]</p><p>CuCl2 + Na2CO3  CuCO3 + 2NaCl</p><p>BaCl2 + H2SO4  BaSO4 + 2HCl</p><p>Page B-4</p>