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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. 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 _____ _






2. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






3. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






4. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






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






7. A state function in which it is the heat content of a substance.






8. 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.


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






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






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






13. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






15. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






16. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.






17. _______ has very little effect on the solubility of liquids or solids in liquid solvents.






18. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.






19. 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.






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






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






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


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






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






25. 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.


26. The heat change during a process carried out at a constant pressure.






27. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






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






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






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. 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.


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






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






35. In an exothermic process - energy is released and ^E of reaction is ________.






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






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






39. A chemical reaction formed from the union of its elements.






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






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






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






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






44. 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.






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






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






47. A hypothetical gas would follow Boyles law under all conditions and is called?






48. Electronegativities _______ as you go down a group.






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






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