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






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






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






4. 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.






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






6. 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.






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






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






9. 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.






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






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






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






13. The vapor pressure increases with increasing _____.






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






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






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






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






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






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






21. Electronegativities _______ as you go down a group.






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






23. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).






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






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






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






27. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _






28. 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.






29. 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.






30. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.






31. 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.






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






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






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






36. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.






37. 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.






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






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






40. 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.






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






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






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






45. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.

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






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






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






49. **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.






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