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






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

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






4. *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.






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






6. 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.






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






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






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






10. 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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11. Rays made up of positive electrodes in basic electron charges.






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






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






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






16. 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.






17. 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.






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






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






20. The vapor pressure increases with increasing _____.






21. 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.






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






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






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






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






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






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






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






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






30. 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).






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






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






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






35. 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.






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






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






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






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






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






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






42. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.






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






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






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






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






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






48. Electronegativities ________ from left to right in a period.






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






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