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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 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.






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






3. 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.






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






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






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






7. 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.






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






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






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






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

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






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






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






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

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






17. 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).






18. *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.






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






20. **Proceeding across a period from left to right - the ionization energy _______.






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






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






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






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






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






26. 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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27. Cells that convert electrical energy into chemical energy.






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






29. 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.






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






31. The energy required to remove an electron from an isolated atom in its ground state.






32. The law stating that in any spontaneous process there is an increase in the entropy of the universe.






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






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






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






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






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






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






41. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.






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






43. 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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44. Rays made up of positive electrodes in basic electron charges.






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






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






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






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






49. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.






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