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

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






3. 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.






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






5. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.






6. 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.






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






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

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






10. 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.






11. 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 _____ _






12. A state function in which it is the heat content of a substance.






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






15. 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






16. 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.






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






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






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






20. 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






21. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge






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






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






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






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






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






27. *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.






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






29. Electronegativities _______ as you go down a group.






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






31. 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.






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






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






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






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






37. 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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38. The freezing point is always lowered by addition of solute.






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






40. *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.






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






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






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






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






45. 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.






46. 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.






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






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






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






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