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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






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






19. 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).






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






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






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






23. Cells that convert electrical energy into chemical energy.






24. 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






25. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






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






27. 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






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






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






30. *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.






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






32. 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.






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






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






35. 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.






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






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






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






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






40. The vapor pressure increases with increasing _____.






41. Metals have electronegativities less than ____






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






43. 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.






44. 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.






45. 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.






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






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






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






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






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