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CLEP Chemistry 1

Subjects : clep, science, chemistry
Instructions:
  • Answer 50 questions in 15 minutes.
  • If you are not ready to take this test, you can study here.
  • Match each statement with the correct term.
  • Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






2. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






3. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






4. Rays made up of electrons in basic electron charges.






5. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _






6. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






7. This process occurs when the system is maintained at the same temperature throughout an experiment.






8. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.






9. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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10. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






11. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






12. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.






13. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.






14. The freezing point is always lowered by addition of solute.






15. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.






16. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






17. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






18. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






19. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






20. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.

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21. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.






22. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

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23. In an endothermic process - energy is absorbed and ^E is _______.






24. The temperature at which a substance's solid and liquid phases are in equilibrium.






25. The most active metals are found in what corner of the periodic table?






26. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






27. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






28. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






29. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.






30. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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31. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






32. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






33. Liquids with strong attractive forces have ______ boiling points.






34. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.






35. This process occurs when the system is thermally isolated so that no heat enters or leaves.






36. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






37. The most active nonmetals are found in what corner of the periodic table?






38. The pressure exerted by each gas in a mixture is called its _____ pressure.






39. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.






40. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.

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41. **Proceeding across a period from left to right - the ionization energy _______.






42. Electronegativities ________ from left to right in a period.






43. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.






44. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






45. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






46. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






47. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






48. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






49. The change in enthalpy of an endothermic reaction is ________.






50. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.