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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. Rays made up of electrons in basic electron charges.






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






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






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






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






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






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

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8. 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.






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






10. 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.






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






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






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






14. 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.






15. 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.






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






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






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






19. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.






20. 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.






21. *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.






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






25. **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.






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






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






28. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






29. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.






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






31. 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).






32. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.






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






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






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






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






37. 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.






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






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






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






42. 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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43. The vapor pressure increases with increasing _____.






44. 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.






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






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






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






48. 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.






49. *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.






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