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






2. *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.






3. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.






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






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






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






7. 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.






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






9. **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.






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






11. Metals have electronegativities less than ____






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






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

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






15. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).






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






17. *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.






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






19. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.






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






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






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






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






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






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






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






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






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






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






32. 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.






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






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






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






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






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






39. 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.






40. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






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






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

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43. The vapor pressure increases with increasing _____.






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






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






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






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






48. 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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49. 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






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