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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 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.






2. *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.






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






4. 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).






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






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






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






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






9. *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.






10. 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).






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






12. Metals have electronegativities less than ____






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






14. 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.






15. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.






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






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






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






19. Cells that convert electrical energy into chemical energy.






20. 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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21. 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.






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






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






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






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






27. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






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






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






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






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






32. When the rate of evaporation equals the rate of condensation - the system is in __________.






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






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






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






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






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






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






39. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.






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






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






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






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






44. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.






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






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






48. 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.






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






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

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