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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. **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.






2. 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.






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






4. 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.






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






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






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






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






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






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






11. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.






12. 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.






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






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






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






16. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.






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






18. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f






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






20. 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.






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






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






23. 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.






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






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






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






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






29. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?






30. 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).






31. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g






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






33. *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.






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






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






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






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






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






41. A hypothetical gas would follow Boyles law under all conditions and is called?






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






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






44. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l






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






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






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






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






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






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