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






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






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






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






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

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






7. 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.






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






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






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






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






14. 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.






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






16. 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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17. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






19. Metals have electronegativities less than ____






20. *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.






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






23. Cells that convert electrical energy into chemical energy.






24. 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.






25. 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.






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






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






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

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






30. 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






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






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






33. 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.






34. 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.






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






36. 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.






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






39. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.






40. 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 _____ _






41. Liquids with strong attractive forces have ______ boiling points.






42. 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






43. *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.






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






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






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






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






50. 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).