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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 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






2. 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.






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






4. 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.






5. 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.






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






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






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






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






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






12. 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.






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






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






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






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






18. 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.






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






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






21. 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.






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






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






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






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






26. 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






27. 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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28. _____ bonds are present in molecules containing double or triple bonds.






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






30. 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).






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






32. 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.






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






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






35. 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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36. The freezing point is always lowered by addition of solute.






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






38. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.






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

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






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






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






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






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






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






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






49. 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.






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