SUMMATIVE-TEST-IN-CHEM.pdf

SUMMATIVE TEST IN GENERAL CHEMISTRY 1. Which of the following gases will effuse most slowly under the same conditions? A. Bromine B. Ammonia (NH3) C. Chlorine D. Hydrogen 2. Based on the definition of diffusion and effusion, which examples are correctly...

SUMMATIVE TEST IN GENERAL CHEMISTRY 1. Which of the following gases will effuse most slowly under the same conditions? A. Bromine B. Ammonia (NH3) C. Chlorine D. Hydrogen 2. Based on the definition of diffusion and effusion, which examples are correctly matched: A. Flat tire: diffusion B. Incense sticks: effusion C. Deflating balloon: diffusion D. Aerosol sprays: effusion 3. Identify the factor that determines rates of diffusion and effusion for different molecules at a given temperature. A. Size of the molecules B. Temperature of the gas C. Molar mass of the gas D. Polarity of the molecules 4. Which of the following is an assumption of the kinetic molecular theory of gases? A. Collisions between gas particles are inelastic B. Gas particles move around in an orderly manner C. Gases consist of closely spaced particles D. The temperature of a gas depends on the average kinetic energy of the gas particles 5. The movement of gas is greatly affected by ___. A. The space of the container B. The temperature of the container C. The size of the container D. The pressure of the container 6. Consider this reaction: 2NaN3 🡪 2 Na + 3 N2. At what pressure (atm) is the nitrogen gas sample that is collected when 48.40 g of NaN3 decomposes? The temperature of the gas is 25.0 degree Celsius, and the volume is 18.40 L. A. 1.25 atm B. 1.49 atm C. 151 atm D. 1,130 atm 7. Following this reaction: MgN2 + 3 H2O 🡪 MgO + 2 NH3. If 10.30 L of ammonia gas at 20.0 degree Celsius and 0.989 atm is created, how many liters of water at STP are required? A. 0.423 L H2O B. 0.204 L H2O C. 14.20 L H2O D. 10.30 L H2O 8. Acetylene is formed by the reaction of water with calcium carbide, according to this equation: CaC2 + H2O 🡪 Ca(OH)2 + C2H2. How many grams of CaC2 would be needed to produce 10.00 L (measured at STP) acetylene? A. 3.50 g CaC2 B. 23.20 g CaC2 C. 25.40 g CaC2 D. 10.30 g CaC2 9. How many moles are in a 22.40 L sample of an Ideal gas STP? A. 1.00 mole B. 0.01 mole C. 0.011 mole D. 10 moles 10. When solving gas stoichiometry problems, which of the following is correctly matched? A. STP conditions; molar mass B. STP conditions; PV=nRT C. Non-STP conditions; PV=nRT D. Non-STP conditions; 22.4 moles 11. What is known as the quantitative study of reactants and products in a chemical reaction. A. Thermochemistry B. Stoichiometry C. Organic Chemistry D. Analytic Chemistry 12. A 5.0 L cylinder contains oxygen gas at 20.00 degree Celsius and 735 mmHg. How many grams of oxygen are in the cylinder? A. 6.40 g O2 B. 3.20 g O2 C. 4.30 g O2 D. 5.10 g O2 13. If a 4.0 L container holds 0.40 moles of Oxygen gas at 350 K. What will be the pressure inside the container? A. 28.70 atm B. 287.00 atm C. 2.87 atm D. 0.287 atm 14. A gas mixture contains 2.5 mol N2 and 9.7 mol CO2, and has a pressure of 2.30 atm. What is the partial pressure of each gas? A. N2 = 1.83 atm; CO2 = 0.47 atm B. N2 = 0.39 atm; CO2 = 1.91 atm C. N2 = 1.91 atm; CO2 = 0.39 atm D. N2 = 0.47 atm; CO2 = 1.83 atm 15. Four gases exert a total pressure of 6 mmHg. Gas A and B exert 2 mmHg each. Gas C exerts 0.20 mmHg. Gas D exerts how much pressure? A. 1.50 mmHg B. 1.80 mmHg C. 2.00 mmHg D. 2.80 mmHg 16. What refers to the pressure each gas exerts in a mixture? A. Half-pressure B. Partial pressure C. Total pressure D. Sum pressure 17. In an Ideal gas, if everything is held constant, doubling the volume will ___ the pressure. A. Double B. Not affect C. Halve D. Eliminate 18. A sample of helium gas has a volume of 0.180 L, a pressure of 0.800 atm and a temperature of 29 degree Celsius. What is the new temperature of the gas at a volume of 90.0mL and a pressure of 3.20 atm? A. 58-degree Celsius B. 331-degree Celsius C. 58 K D. 331 K 19. A hydrogen balloon has an initial pressure of 1.50 atm and is inflated from 2L to 6L. What is the final pressure of this balloon after it is inflated? A. 0.50 atm B. 2.00 atm C. 8.00 atm D. 10.50 atm 20. With pressure constant, the temperature of a gas is increased from 30 degree Celsius to 90 degree Celsius. The volume will ___? A. Increased by about 20% B. Decreased by half C. Triple D. Remain the same 21. If you collect 22.4 L of Oxygen gas at standard conditions, you will have ____. A. 1 mole of gas B. 32 g of gas C. 6.02 x 10^23 molecule of gas D. All of these answers 22. The pop-up timer is a device designed to let you see visually when a piece of meat has reached a certain state of doneness during cooking. This instrument uses what kind of gas law? A. Boyle’s Law B. Charles’ Law C. Gay-Lussac’s Law D. Avogadro’s Law 23. Two ways to increase pressure are: A. Increase both force and surface area B. Decrease both force and surface area C. Decrease force and increase surface area D. Increase force and decrease surface area 24. Consider this reaction: LiOH + KCl 🡪 LiCl + KOH. A scientist began this reaction with 20 grams of lithium hydroxide and an unlimited amount of KCl. The reaction actually produced 6 grams of lithium chloride. What is the percent yield? A. 15 % B. 16 % C. 17 % D. 18 % 25. Using this reaction: 3FeCl2 + 2Na3PO4 🡪 Fe3(PO4)2 + 6NaCl. If 23 g of Iron (II) chloride reacts with 41 g of sodium phosphate, what is the limiting reagent? A. FeCl2 B. Na3PO4 C. Fe3(PO4)2 D. NaCl 26. With the same reaction from the previous question, how much sodium chloride can be formed? 3FeCl2 + 2Na3PO4🡪 Fe3(PO4)2 + 6NaCl. A. 18 g NaCl B. 21 g NaCl C. 25 g NaCl D. 44 g NaCl 27. The complete reaction of 10.56 g NH3 is expected to produce 21.80 g of urea. The amount of urea produced in the reaction is 16.22 g. What is the theoretical yield? A. 5.66 g B. 16.22 g C. 10.56 g D. 21.80 g 28. A reaction was predicted to produce 43.50 grams of a compound. When the product was measured, there were only 26.10 grams made. What is the percent yield? A. 60.00 % B. 17.40 % C. 69.60 % D. 166 % 29. Which of the following best describes excess and limiting reagent? A. Limiting reagent remains at the end of the reaction while excess reagent runs out. B. Limiting reagent limits the amount of product and excess reagent remains at the end of reaction. C. Both excess and limiting reagents run out by the end of reaction. D. Excess reagent limits the amount of product and limiting reagent limits the amount of reactant. 30. Consider the equation below: HNO3+NaHCO3 🡪 NaNO3+H2O+CO2. Determine the total mass of H2O+CO2 produced when 5.73 g of NaHCO3 reacted completely with excess HNO3. A. 1.23 g B. 3.00 g C. 4.23 g D. 5.93 g 31. The combustion of pentane gives as this following reaction: C5H12 + O2 🡪 CO2 + H2O. Calculate how many moles of O2 would be required for the complete reaction of 3.50 moles of pentane? a. 0.438 mol O2 b. 28.00 mol O2 c. 2.29 mol O2 d. 0.545 mol O2 32. Using the same reaction as the previous question, how many grams of H2O will be produced starting with 5.00 moles of pentane? a. 5.63 g H2O b. 1,440 g H2O c. 1.67 g H2O d. 540 g H2O 33. Consider the balanced equation below: 2LiOH + CO2 🡪 Li2CO3 + H2O. Construct the mass ratio for LiOH. a. 24 g LiOH / 1 mol LiOH b. 24 g Li OH / 2 mol LiOH c. 48 g LiOH / 1 mol LiOH d. 48 g LiOH / 2 mol LiOH 34. Consider the balanced equation below: Cu + 2AgNO3 🡪 Cu(NO3)2 + 2Ag. Determine the mole ratio between AgNO3 and Ag. a. 1 mol Ag / 1 mol AgNO3 b. 1 mol Ag / 2 mol AgNO3 c. 2 mol Ag / 1 mol AgNO3 d. 2 mol Ag / 2 mol AgNO3 35. Copper nitrate can be formed from a copper interacting with a nitric acid. Balance this following reaction: _Cu + _HNO3 🡪 _Cu(NO3)2 + _NO + _H2O a. (1,4,1,1,2) b. (3,6,1,2,4) c. (3,8,3,2,4) d. (1,4,2,1,2) 36. Balance the following equation: _SeCl6 + _O2 🡪 _SeO2 + _Cl2 a. (1,1,1,3) b. (1,2,1,2) c. (2,1,2,1) d. (2,2,2,4) 37. Tetraphosphorus decoxide reacts with water and it yields to phosphoric acid. Write and balance the chemical equation, then identify what will be the coefficient of water. a. 4 b. 6 c. 8 d. 10 38. Which of the following equations are correctly balanced? a. 12CO2 + H2O 🡪 C6H12O6 + O2 b. CO2 + H2O 🡪 3C6H12O6 + O26 c. 6CO2 + 6H2O 🡪 C6H12O6 + 6O2 d. CO2 + 9H2O 🡪 C6H12O6 + O2 39. Sodium oxide reacts with water to produce sodium hydroxide. What is the appropriate chemical equation? a. NaO + H2O 🡪 NaOH b. Na2O + H2O 🡪 NaOH c. NaO2 + H2O 🡪 NaOH d. NaO + H2O 🡪 Na2OH 40. What type of reaction is this? Pb(NO3)2 + KI 🡪 PbI2 + KNO3. a. Synthesis b. Decomposition c. Single Displacement d. Double Displacement 41. There is an acid that is added to food as a mold inhibitor. Its composition is 64.30% of C, 7.20% of H, and 28.50% of O, and its molar mass is 112 g/mol. What is its molecular formula? a. C2H2O b. C8H6O2 c. C3H4O d. C6H8O2 42. How many grams of Iron can be recovered from a 115 g sample of Ferric carbonate? a. 38.40 g b. 44.10 g c. 19.20 g d. 22.10 g 43. What percent of AgNO3 is Silver? a. 60% b. 62% c. 64% d. 66 % 44. The sample was found to contain 79.80% C and 20.20% H. Determine its Empirical formula. a. CH b. CH2 c. CH3 d. CH4 45. Find the percentage composition of Copper (I) sulfide. a. Cu = 88.89% ; S = 11.11% b. Cu = 80% ; S = 20% c. Cu = 67.99% ; S 32.01% d. Cu = 60 % ; S = 40% 46. Which of the following is the correct chemical formula for sodium hydrochlorite. a. NaClO b. NaClO2 c. NaClO3 d. NaClO4 47. What is the correct name for this compound: CS a. Carbon monosulfite b. Carbon monosulfide c. Carbon sulfide d. Carbon sulfite 48. What is the name of this compound: VI3. a. Vanadium triiodide b. Vanadium iodide c. Vanadium (II) iodide d. Vanadium (III) iodide 49. The name given for a straight chain hydrocarbon with seven carbon atoms is ____. a. Nonane b. Hexane c. Heptane d. Octane 50. Among chemical formulas shown, which represents the compound with the greatest number of ions? a. AICl3 b. KI c. BaCl2 d. (NH4)2SO4 51. Which of the following is an example of an empirical formula? a. C2H4 b. PH5 c. H2O2 d. Hg2Cl2 52. Which is a chemical formula for an ionic compound? a. AsH3 b. CH4 c. KCl d. H2Se 53. Which of the following statements are true? a. Atoms of the same element always have the same mass number. b. Atoms with same atomic number are always isotopes. c. Atoms with the same mass number are always isotopes. d. Atoms of the same element can have different mass numbers. 54. All of the following are common names of isotopes of hydrogen except? a. Hydronium b. Deuterium c. Protium d. Tritium 55. Which pair of mixture and separation method correspond to one another? a. copper filings and sand; filtration b. milk; centrifugation c. oil and water; distillation d. sand and water; magnetic separation 56. If you shake up the sand and water, the sand spreads through the water forming cloudy _____. a. Colloid b. Solution c. Sediment d. Suspension 57. A process in which mixture is passed through a media and is separated through differences in the rates at which the components migrate is known as ___. a. Filtration b. Chromatography c. Distillation d. Evaporation 58. A 14-karat gold is an example of what classification of matter? a. Element b. Pure Substance c. Homogeneous mixture d. Heterogeneous mixture 59. Which of the following does NOT signal a chemical change? a. Change in state b. Production of gas c. Color change d. Production of light and heat 60. AYOQ N