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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. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






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






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






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






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






6. 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.






7. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






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






9. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






10. 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 _____ _






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






12. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






14. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.






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






16. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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17. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.






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






19. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.






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






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






22. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f






23. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.






24. The heat required to change 1mole of solid completely to vapor.






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






26. _____ bonds are present in molecules containing double or triple bonds.






27. 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.






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






29. Electronegativities _______ as you go down a group.






30. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.






31. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






32. 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.






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






34. 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.






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






36. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.






37. 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).






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






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






41. 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.






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






43. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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44. In titration - this is the point at which a particular indicator changes color.






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. When the electron moves from the ground state to an excited state - it ______ energy.






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






48. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.






49. The molecules in a gas are in constant - continueous - random - and straight-line motion.






50. Metals have electronegativities less than ____