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






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






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






4. 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.






5. 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).






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






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






9. 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.






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






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






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






13. Electronegativities ________ from left to right in a period.






14. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.






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






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






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






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






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






20. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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21. Metals have electronegativities less than ____






22. 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 _____ _






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






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






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






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

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27. 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






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






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






30. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






31. 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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32. The change in enthalpy of an endothermic reaction is ________.






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






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






35. The solubility of gases in liquid or solid solvents always increases with ________ pressure.






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






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






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






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






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






41. 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.






42. 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.






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






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






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






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






47. 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.






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

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






50. Cells that convert electrical energy into chemical energy.







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