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






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






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






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






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






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






7. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.






8. *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.






9. 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).






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






12. 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






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






14. Liquids with strong attractive forces have ______ boiling points.






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






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






17. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






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






24. Electronegativities _______ as you go down a group.






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






26. 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.






27. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






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






29. 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.






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






31. 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 _____ _






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






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






34. *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.






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






37. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






38. Metals have electronegativities less than ____






39. 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.






40. 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.






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






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






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






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






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






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






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






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






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






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