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Quick Mid Term Review

Quick Mid Term Review. Multiple Choice Questions! . Which of the following is not a pure substance?. water carbon dioxide carbon d. air. Solutions may be. solids. liquids. gases. d. All of the above. Explain the difference between a scientific law (X) and a scientific theory (Y).

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Quick Mid Term Review

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  1. Quick Mid Term Review Multiple Choice Questions!

  2. Which of the following is not a pure substance? water carbon dioxide carbon d. air

  3. Solutions may be solids. liquids. gases. d. All of the above

  4. Explain the difference between a scientific law (X) and a scientific theory (Y). X = is proven; Y = is not proven X = is not proven; Y = is proven X = tells what happens; Y = explains why things happen X = explains why things happen; Y = tells what happens

  5. Properties that describe the way a substance reacts to form other substances are called physical properties. chemical properties. homogeneous properties. d. heterogeneous properties.

  6. When nitric acid is mixed with copper metal, a brown gas forms. This is an example of an accident. a chemical reaction. a physical property. d. an extensive property.

  7. Heat flows from an object at high temperature to an object at low temperature. at low temperature to an object at high temperature. to another object at the same temperature. d. at high elevation to an object at low elevation.

  8. The nucleus of an atom contains protons and neutrons. protons and electrons. electrons and neutrons. d. air.

  9. Two atoms with the same atomic number but different mass numbers are called mutants. isomers. isotopes. d. symbiots.

  10. The elements found on the left side of the periodic table tend to ______ electrons. gain lose keep d. share

  11. A metal and a nonmetal react to form ________ compound. a molecular a mixed an empirical d. an ionic

  12. Compounds composed only of carbon and hydrogen are called binary acids. carbohydrates. hydrocarbons. d. alkanes.

  13. Which of the formulas below does not represent a compound that actually exists? CaCO3 H2O2 KMnO4 d. Na2PO3

  14. NaOCl is named sodium chlorate. sodium chlorite. sodium perchlorate. d. sodium hypochlorite.

  15. LiNO3 is named lithium nitrate. lanthanum nitrate. lanthanum nitrite. d. lithium nitrite.

  16. Cl2O7 is named chlorine(VII) oxide. dichlorine hexaoxide. dichlorine heptaoxide. d. bichlorine heptaoxide.

  17. Hydrocarbons burn to form H2O and CO2. charcoal. methane. d. O2 and H2O.

  18. C6H6 + O2 CO2 + H2OWhen this equation is correctly balanced, the coefficients are 1, 7  6, 3. 1, 8  6, 3. 2, 15  12, 6. d. 2, 16  12, 6.

  19. 2 NaN3 2 Na + 3 N2This is an example of a _______ reaction. decomposition combination combustion d. replacement

  20. The percentage by mass of phosphorus in Na3PO4 is 44.0. 11.7. 26.7. d. 18.9.

  21. Ribose has a molecular weight of 150 grams per mole and the empirical formula CH2O. The molecular formula of ribose is C4H8O4. C5H10O5. C6H14O4. d. C6H12O6.

  22. A homogeneous mixture of two or more components is referred to as a solute. a solution. an electrolyte. d. a mess.

  23. The solvent in a sample of soda pop is sugar. carbon dioxide. water. d. air.

  24. Gatorade conducts electricity because it contains water. sugar. air. d. electrolytes.

  25. When Fe(NO3)2 dissolves in water, the particles in solution are Fe+ and (NO3)2-. Fe2+ and 2 NO3-. Fe and 2 NO3. d. Fe and N2 and 3 O2.

  26. As a helium-filled balloon rises, its volume increases. This is an example of _______ Law. Avogadro’s Boyle’s Charles’s d. Gay-Lussac’s

  27. Avogadro’s Law states that the volume of a sample of a gas is proportional to the _______ of the gas. number of moles mass pressure d. temperature

  28. Standard temperature and pressure (STP) equals (X) atmosphere(s) and (Y) degrees Celsius. X = 0, Y = 25 X = 1, Y = 0 X = 1, Y = 25 d. X = 0, Y = 0

  29. A sample of 2.0 moles of nitrogen (N2) gas at STP occupies a volume of _______ liters. 11.2 22.4 44.8 d. 89.6

  30. The partial pressure of each gas in a mixture of gases is proportional to the _______ of the gas. mass molecular weight square root of the molecular weight d. mole fraction

  31. The kinetic-molecular theory of gases states that the average kinetic energy of the gas particles is proportional to the _______ of the gas. Kelvin temperature Celsius temperature number of moles d. pressure

  32. Neon gas undergoes effusion _______ krypton gas does. slower than at the same rate as twice as fast as d. four times as fast as

  33. A gas is most likely to exhibit ideal behavior at (X) temperature and (Y) pressure. X = low, Y = low X = low, Y = high X = high, Y = low d. X = high, Y = high

  34. Which gas below has the greatest density at STP? Ne Ar Kr d. Xe

  35. The rate of a reaction can be increased by increasing reactant concentrations. increasing the temperature. adding a suitable catalyst. d. All of the above

  36. Over time, the rate of most chemical reactions tends to _______. increase decrease remain constant d. oscillate

  37. If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A. zeroth first second d. third

  38. Reaction: A + B  C + DRate = k[A][B]The overall order of this reaction is first. second. third. d. fourth.

  39. Reaction: W + X  Y + ZRate = k[W]The order of this reaction with respect to X is zeroth. first. second. d. third.

  40. The time required for the concentration of a reactant to be reduced to half of its initial value is called the midpoint of the reaction. equivalence point of the reaction. half-rate of the reaction. d. half-life of the reaction.

  41. The rate-determining step is the _______ step in a reaction mechanism. first last c. fastest d. slowest

  42. Adding a catalyst increases the rate of a chemical reaction because the presence of the catalyst increases molecular velocities. increases molecular collisions. decreases energy of activation. d. All of the above

  43. At equilibrium, the rate of the forward reaction is _______ the rate of the reverse reaction. equal to slower than faster than d. the reverse of

  44. The reaction quotient Q is usually represented by [reactants] / [products]. [products] / [reactants]. [reactants]  [products]. d. [reactants] + [products].

  45. If the value of the equilibrium constant is large, then _______ will mostly be present at equilibrium. reactants products catalysts d. shrapnel

  46. Q = the reaction quotientK = the equilibrium constantAt equilibrium, which is true? Q > K Q < K Q = K d. Q2 = K

  47. CO2 + H2 CO + H2OIf all species are gases and H2 is added, the concentration of CO at equilibrium will increase. decrease. remain unchanged. d. disappear.

  48. CO2 + H2 CO + H2OIf all species are gases and H2O is added, the equilibrium concentration of CO will increase. will decrease. will remain unchanged. d. will disappear.

  49. CO2 + H2 CO + H2OIf all species are gases and CO2 is removed, the [CO] at equilibrium will increase. decrease. remain unchanged. d. disappear.

  50. CO2 + H2 CO + H2OIncreasing the temperature of this endothermic reaction will _______ [CO] at equilibrium. increase decrease not change d. eradicate

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