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






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






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






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






5. Cells that convert electrical energy into chemical energy.






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






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






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






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






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






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






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






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






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






15. 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






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






17. 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.

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






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






20. 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.






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






22. 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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23. *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.






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






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






26. Rays made up of positive electrodes in basic electron charges.






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






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






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






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






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






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






33. 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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34. 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.






35. The heat required to change 1mole of solid completely to vapor.






36. The molecules in a gas are in constant - continueous - random - and straight-line motion.






37. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.






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






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






40. 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.






41. *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.






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






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






45. Electronegativities _______ as you go down a group.






46. 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.






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






48. 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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49. 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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50. 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.