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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 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.






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






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






4. 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.






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






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






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






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






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






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






11. *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.






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






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






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






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






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






18. Metals have electronegativities less than ____






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






20. 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 _____ _






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






22. *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.






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






24. 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.






25. 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.






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






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






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






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






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






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






32. 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.






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






34. The vapor pressure increases with increasing _____.






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






36. 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.






37. 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.






38. 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.






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






40. When an electron moves from an excited state to the ground state - it _______ energy.






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






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






43. *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






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






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






46. 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.






47. 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.






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






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






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