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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. 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.






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






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






4. 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.






5. The vapor pressure increases with increasing _____.






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






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






8. Cells that convert electrical energy into chemical energy.






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






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






11. 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.






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






13. 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.

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14. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.






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






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






17. 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.






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






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






20. *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.






21. A solution in which solid solute is in equilibrium with dissolved solute.






22. Metals have electronegativities less than ____






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






24. 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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25. 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.






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






27. 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.






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






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






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






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






32. 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).






33. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.

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






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






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






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






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






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






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






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






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






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






44. Electronegativities _______ as you go down a group.






45. The most active metals are found in what corner of the periodic table?






46. 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.






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






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






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






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







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