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






2. 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.






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






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






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






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






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






8. 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.






9. 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.






10. *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.






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






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






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






14. 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.






15. 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).






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






17. 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.






18. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.






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






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






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






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






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






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






25. **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.






26. 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.






27. Metals have electronegativities less than ____






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






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






30. 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.






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






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






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






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






35. Electronegativities _______ as you go down a group.






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






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






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






39. 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.


40. 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.






41. When the rate of evaporation equals the rate of condensation - the system is in __________.






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






43. 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.






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






45. 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.


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






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






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






49. 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






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