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Quiz I 1. Get the conversion factor for the unit of surface area from 1 mm = 10-6 m (1 mm)2 = (10-6 m)2 1 mm2 = (10-12 m2 2. Write the conversion ratios for the 1 lb = 453.6 g conversion factor 1 lb / 453.6 g , 453.6 g / 1 lb 3. Convert 1.23 x 1022 pm3 to in3 . 1.23 x 1022 pm3 x ( 10-12 m / 1pm)3 x ( 1 cm / 10-2 m )3 x ( 1 in / 2.54 cm)3 = 7.5 x 10-8 in3 4. A solid sample has the density of 11.22 g/ ml. and mass of 8.902 g. Calculate volume off the solid sample. 8.902 g x ( 1 ml. / 11.22 g) = 0.7934 ml. 5. Convert 112.5 o F to o C. o F = 1.8 x o C + 32 o C =( o F - 32) / 1.8 o C = (112.5 o F - 320 / 1.8 44.7 o C 6. Which of the following substances is element/ compound? a. CO : compound b. B2O3 : compound c. Fe : element Quiz II 1. Complete the following table:
2. Find name and symbol of an atom in period 3 and VIA group. Sulfur, S
3. An atom has the atomic number of 42, find the period and group. Period 5, B (transition group) 4. Complete the following table:
Quiz III 1. Write the formula of each of the following compounds: a. chromium (III) sulfate: Cr2(SO4)3 b. potassium iodide: KI c. diphosphorus trioxide: P2O3 d. chlorous acid: HClO2 (aq) 2. Write the Stock-system name of the following compounds: a. FeO : iron (II) oxide b. Al(HCO3)3: aluminum hydrogen carbonate c. SiO2: silicon dioxide d. HI(aq): hydroiodic acid 3. A compound has 59.63%Cl and 40.4% O. Calculate the empirical formula. moles of Cl: 59.63 g Cl x (1mole Cl / 35.45 g Cl) = 1.682 moles of O : 40.4 g O x ( 1mole O / 16.00 g O) = 2.53 1.682 moles Cl / 1.682 = 1.000 moles Cl 2.53 moles O / 1.682 = 1.50 moles O 1.000 moles Cl x 2 = 2.000 moles Cl 1.50 moles O x 2 = 3.00 moles O empirical formula: Cl2O3 4. Balance the following chemical equation: 2Cr(s) + 6HCl (aq) ------- > 2CrCl3 (aq) + 3H2 (g) 5. Identify the type of the following chemical reaction: H2SO3(aq) ---------- > SO (g) + H2O decomposition reaction Quiz IV: 1. Consider the following chemical reaction: CaC2(s) + 2H2O --------- > Ca(OH)2 (s) + C2H2 (g) 11.2 g CaC2 react with excess of water, calculate the theoretical yield of C2H2. 11.2 g CaC2 x ( 1mole / 64.10 g CaC2) x (1mole C2H2/ 1mole CaC2) x (26.04 g C2H2 / 1 mole C2H2) = 4.55 g C2H2 2. Refer to problem #1 if 1.340 g C2H2 have been recovered, calculate the %yield. %yield = (1.340 g C2H2 / 4.55 g C2H2) x 100 = 29.5% 3. 44.67 g iron absorbs 266 J of heat and its temperature is increased by 23.0 oC. calculate the specific heat of iron. Q = m x s x Dt Dt = t2 - t1 s = Q / ( m Dt ) s = 266 J / ( 44.67 g x 23.0 oC) s = 0.260 J / g oC 4. Write the complete electronic configuration of an atom having atomic number of 22. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d2 5. Refer to problem number 4 is the atom in the main group or transition group? transition group Quiz V: 1. Draw the Lewis structure of COCl2: : O : .. | | .. : Cl - C - Cl : .. .. 2. Determine the molecular shape of COCl2: trigonal planar 3. A sample of gas has the volume of 33.4 L. with the pressure of 3.45 atm. at 22 oC. Calculate the volume at STP P1V1 / T1 = P2V2 / T2 V2 = P1V1T2 / T1P2 T1 = 11 oC + 273 = 295 K T2 = 0 oC + 273 = 273 K V2 = (3.45 atm. x 33.4 L. x 295 K) / (273 K x 1.00 atm.) V2 = 107 L. 4. Consider the following chemical reaction: N2 (g) + 3H2 (g) ------ > 2NH3 (g) 1.70 g ammonia gas has been obtained. Calculate volume of of H2(g) at 25 oC and pressure of 11.4 atm. g of NH3 ----------------- > moles of NH3 -------------- > moles of H2 1.70 g NH3 x (1mole NH3 / 17.02 g NH3) x ( 3 moles H2 / 2 moles NH3) = 0.150 moles H2 PV = nRT V = nRT / P T = 25 oC + 273 = 298 K V = (0.150 moles x 0.0821 atm. L. mole -1 K-1 x 298 K) / 11.4 atm. V = 0.322 L. 5. Calculate the amount of heat to vaporize 10.2 g water at its boiling point. 10. g H2O x ( 1mole H2O / 18.02 g H2O) x (40.7 kJ / 1 mole H2O) = 23.0 kJ
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