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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. 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.






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






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






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






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






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






9. Cells that convert electrical energy into chemical energy.






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






11. 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.






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






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






14. Electronegativities _______ as you go down a group.






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






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






17. 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






18. The vapor pressure increases with increasing _____.






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






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






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






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






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






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






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






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






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






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






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






31. 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.






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






33. *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.






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






35. 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.






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






37. Metals have electronegativities less than ____






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






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

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






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






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






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






45. The freezing point is always lowered by addition of solute.






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






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






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






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






50. 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.