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






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






3. *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.






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






6. *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.






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






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






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






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






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






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






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






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






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






16. 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.






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






18. *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.






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






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






22. 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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23. The change in enthalpy of an endothermic reaction is ________.






24. 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.






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

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26. When an electron moves from an excited state to the ground state - it _______ energy.






27. 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.






28. 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.






29. 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).






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






31. 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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32. 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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33. In an endothermic process - energy is absorbed and ^E is _______.






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






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






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






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






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






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






40. 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.






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






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






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






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






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






46. When the electron moves from the ground state to an excited state - it ______ energy.






47. Electronegativities _______ as you go down a group.






48. Heat added to a system and work done by a system are considered _________ quantities.






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






50. 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.