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






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






4. 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.






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






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

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






8. Electronegativities _______ as you go down a group.






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






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






12. 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).






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






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






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






16. 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.






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






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






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






20. 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.






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






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






23. The most active nonmetals are found in what corner of the periodic table?






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






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






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






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






28. Cells that convert electrical energy into chemical energy.






29. 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.






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






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






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






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






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






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






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






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






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






39. The vapor pressure increases with increasing _____.






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






41. 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.






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






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






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






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






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






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






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






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






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