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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. 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.






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






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






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






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






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






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






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






9. Cells that convert electrical energy into chemical energy.






10. 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).






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






12. The vapor pressure increases with increasing _____.






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






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






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






16. 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.






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






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






19. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






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






21. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.






22. 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.






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






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






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






26. 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).






27. 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






28. 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.






29. 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.






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






31. Electronegativities _______ as you go down a group.






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






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






34. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






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






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






38. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.






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






40. 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.






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






42. 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 _______.






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






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






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






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






47. 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.






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






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






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