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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 temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






2. The action of salts of weak acids or bases with water to form acidic or basic solutions.






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






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






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






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






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






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






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






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






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






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






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






15. Electronegativities _______ as you go down a group.






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






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






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






19. 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






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






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






22. 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).






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






24. 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 _____ _






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






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






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






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






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






30. 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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31. 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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32. 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






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






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






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






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






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






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






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






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

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42. *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.






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






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






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






46. Cells that convert electrical energy into chemical energy.






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






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






49. Metals have electronegativities less than ____






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







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