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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 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.






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






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






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






5. *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.






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






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






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






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






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






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






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






14. 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.






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






17. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






18. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.






19. 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.






20. 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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21. The vapor pressure increases with increasing _____.






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






23. 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.






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






25. 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.






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






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






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






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






30. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






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






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






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






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






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






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






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. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






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






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






41. 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.






42. 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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43. 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.






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






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






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






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






48. Cells that convert electrical energy into chemical energy.






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






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






Can you answer 50 questions in 15 minutes?



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