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






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






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






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






5. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






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






7. 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).






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






9. 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.






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






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






12. 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.






13. 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.






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






15. 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.


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






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






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


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






20. 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.


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






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






23. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






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






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






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






27. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






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






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






30. 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.






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






32. 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 _____ _






33. Electronegativities _______ as you go down a group.






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






35. Metals have electronegativities less than ____






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






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






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






39. The vapor pressure increases with increasing _____.






40. **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.






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






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






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






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






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






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






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






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






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






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