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






2. 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.






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






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






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






6. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






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






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






10. 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.

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11. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






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






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






14. 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.






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






16. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f






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






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

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






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






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






22. 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.






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






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






25. *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.






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






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






28. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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






30. 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.






31. 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.






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






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






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






35. 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.






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






37. **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.






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






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






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






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






42. Cells that convert electrical energy into chemical energy.






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






44. 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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45. 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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46. The heat change during a process carried out at a constant pressure.






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






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






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