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






2. 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.






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






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






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






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






7. 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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8. 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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9. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






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






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






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






14. 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.






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






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






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






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






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






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






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






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






23. 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.






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






25. 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 _____ _






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

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






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






29. *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.






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






31. The energy required to remove an electron from an isolated atom in its ground state.






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






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






34. 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.






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






36. 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.






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






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






39. Cells that convert electrical energy into chemical energy.






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






42. **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.






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






44. 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






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






46. The vapor pressure increases with increasing _____.






47. 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.






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






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






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