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






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






3. Cells that convert electrical energy into chemical energy.






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






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

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






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






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






11. 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.






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






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






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






15. 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.






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






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






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






19. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____






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






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






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






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






24. *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.






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






26. 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.






27. 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






28. Metals have electronegativities less than ____






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






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






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






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






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






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






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






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






37. 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).






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






39. 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.






40. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.






41. 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






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






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






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






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

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






47. **Proceeding across a period from left to right - the ionization energy _______.






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






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