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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. **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.






2. 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.


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






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






5. 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.






6. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






7. 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.


8. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






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






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






11. The vapor pressure increases with increasing _____.






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






13. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






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






15. 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.






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.


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


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






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






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






21. 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.






22. *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.






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






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






25. Heat added to a system and work done by a system are considered _________ quantities.






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






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






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






29. 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






30. 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.






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






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






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






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






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






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






37. 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.






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






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






40. 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.






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






42. 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 _____ _






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






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






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






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






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






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






49. 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.






50. Metals have electronegativities less than ____