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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. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.

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2. Deviations from Boyles law that occur with real gases represent _______ behavior.






3. 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.






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






5. Electronegativities _______ as you go down a group.






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






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






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






10. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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






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






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

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14. 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.






15. 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 _____ _






16. 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).






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






18. 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.






19. Rays made up of positive electrodes in basic electron charges.






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






21. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.






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






23. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






25. 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.






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






27. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






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






29. 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.






30. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






31. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






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






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






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






35. The change in enthalpy of an exothermic reaction is ________.






36. A process that occurs whent eh system is maintained at constant pressure.






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






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






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






40. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.






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






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






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






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






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






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






47. 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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48. The energy required to remove an electron from an isolated atom in its ground state.






49. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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