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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. 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.






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






3. 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.






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






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






6. 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).






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






8. 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.






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






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






12. Cells that convert electrical energy into chemical energy.






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






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






15. 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.






16. 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.






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






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






19. 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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20. The vapor pressure increases with increasing _____.






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






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






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






24. 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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25. 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.






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






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






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






29. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?






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






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






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






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






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






35. **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.






36. 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






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






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






39. 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 _____ _






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






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






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






43. 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






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






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






46. 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.






47. 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






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






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

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50. *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.