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Liquids and Solids Review Game

Hydrogen bonding is not important in

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Liquids and Solids Review Game

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    1. Liquids and Solids Review Game Honors Chemistry

    2. Hydrogen bonding is not important in ice formation the liquid properties of water dissolving ammonia to water liquid CH4 liquid HF

    3. For the reaction A + B ? C ?Ho = +30 kJ; ?So = +50 J/K. Therefore the reaction is: spontaneous at all temperatures nonspontaneous at all temperatures spontaneous at temperatures less than 600 K spontaneous at temperatures greater than 600K spontaneous only at 25oC.

    4. Which one of the following statements is incorrect? Dispersion (London) forces are the weakest type of intermolecular interactions The strong intermolecular attractions in H2O result from hydrogen bonding The boiling point of H2S is lower than H2O The boiling point of non-polar substances tends to decrease with increasing molecular weight None of the above is incorrect

    5. A white substance melts with some decomposition at 730oC. As a solid, it is a nonconductor of electricity but it dissolves in water to form a conducting solution. The white substance is: a covalent network solid an ionic solid a molecular solid a metallic solid solid Ar

    6. Drops of water and ethanol are placed on a warm stove, and the ethanol drop is seen to evaporate more rapidly. The graph below includes the vapor pressure of ethanol and water. Which curve corresponds to ethanol? A B C D none of the above

    7. The triple point is: the point in a phase diagram where the solid, liquid, and gas phases of a substance coexist at equilibrium the point where all three phases are unstable three places in a phase diagram where the solid, liquid and gas can coexist a three-dimensional phase diagram a rare play in baseball

    8. What happens to molecules in a liquid when the liquid is heated and vapor starts to form? the intramolecular forces between liquid molecules are disrupted the intermolecular forces between liquid molecules are disrupted kinetic energy is removed from the system London forces become stronger surface tension increases, which causes beading up, then boiling

    9. Calculate ?S0 for the reaction below at 25C. S0 for SiH4 = 204.5 J/molK, for O2(g) = 205.0 J/molK, for SiO2 (s) =41.84 J/molK, for H2O(l) = 69.91 J/molK SiH4 (g) + 2O2(g) ? SiO2(s) + 2H2O(l) -353.5 J/K - 432.8 J/K 595.0 J/K -677.0 J/K -880.3 J/K

    10. Which of the following has the strongest intermolecular forces? O2 Ar CH2 HF HBr

    11. What pressure would be required to liquify (or condense) a sample of water vapor at 500oC? 0.0060 atm 1.00 atm 218 atm some pressure higher than 218 atm but which cannot be determined from the phase diagram no amount of pressure can bring about the change of H2O vapor to liquid at 500oC

    12. When a liquid vaporizes, all but one of the following changes occur. Which one does NOT occur? Distance between molecules increases Attractive forces between molecules become less important Density decreases Composition of molecules changes

    13. Which one of the following quantities would you expect to be largest for a given substance? Heat of vaporization per mole Heat of fusion per mole Heat of vaporization per gram Heat of fusion per gram

    14. A solid with a high melting point but no electrical conductivity is: Ionic Molecular Metallic Covalent network

    15. As the pressure increases, the melting point of compound X will: decrease and then increase increase and then decrease decrease increase stay the same

    16. Which of the following is NOT characteristic of a metal? High conductivity High water solubility Low ionization energy Forms positive ions

    17. Which of the following molecules would NOT show hydrogen bonding? CH3NH2 (CH3) 2NH CH3CH2NH2 (CH3) 3N

    18. What is the specific heat of iron if 45.0g of iron metal at 95.0C are dropped into 200.g of water at 25.0C and the temperature of water rises to 28.0C? 0.199 cal/gC 1.99 J/gC 0.199 kJ/gC 1.99 cal/gC None of the above

    19. Which of the following reactions is likely to have the most positive change in entropy? N2(g) + 3H2(g) ? 2NH3(g) CaO(s)+CO2(g) ? CaCO3(s) N2(g)+2O2(g) ? 2NO2 (g) C(s)+)O2(g) ? CO2(g) 2C(s)+O2(g) ? 2CO(g)

    20. The cooling curve below shows how the temperature of a sample varies with time as the sample goes through phase changes. The sample starts as a gas, and heat is removed at a constant rate. At which time does the sample contain the most liquid? t1 t2 t3 t4 t5

    21. How much energy is needed to convert 50.0 g of ice at -5.00C to water at 25C? Specific heat (ice) = 2.10 J/(gC) Specific heat (water) = 4.18 J/(gC) Heat of fusion = 333 J/g Heat of vaporization = 2258 J/g 175 J 22.4 kJ 21.9 kJ 37.3 kJ 18.0 J

    22. Which of the following statements are false? 1. Liquids with large intermolecular forces tend to have very low boiling points 2. Liquids with large intermolecular forces tend to have considerable surface tension 3. When a substance changes from a solid to a liquid, the molecules remain intact 4. The hardness of diamond is due to strong dipole-dipole attraction 1 and 4 1 and 3 2 and 3 2 and 4 3 and 4

    23. Answers D D D B A A B B D E D A D D B D A E D B A

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