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






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






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






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






6. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






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






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






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






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






11. 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.






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






13. Cells that convert electrical energy into chemical energy.






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






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






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






18. 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






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






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






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






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






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






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






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






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






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






30. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






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






32. 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).






33. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






34. 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.






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






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

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






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






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






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

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41. 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.






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






43. Electronegativities _______ as you go down a group.






44. *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.






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






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






47. 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).






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






49. 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.






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