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






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






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






4. 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.

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






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






7. 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.

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8. 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.






9. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.

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

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






12. 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.






13. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.






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






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






16. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






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






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






19. **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.






20. 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.






21. The vapor pressure increases with increasing _____.






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






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






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






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






26. 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.






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. 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.






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

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






32. 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.






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






34. 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.






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






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






37. 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).






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






39. Cells that convert electrical energy into chemical energy.






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






41. 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.






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






43. 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.






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






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






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






47. 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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48. 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 _____ _






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






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