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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 change in enthalpy of an exothermic reaction is ________.






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






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






4. 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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5. 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.






6. *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.






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






8. 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.






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






10. 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).






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






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






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






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

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






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

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






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






19. 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 _____ _






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






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






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






24. 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.






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






26. 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.






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






28. The vapor pressure increases with increasing _____.






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






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






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






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






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






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






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






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






37. 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






38. 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.






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






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






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






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






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






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






45. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.






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






47. 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.






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






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






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