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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 ______ 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).






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






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






4. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.






5. 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.






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






7. 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 _____ _






8. 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






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






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






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






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






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






14. 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.






15. 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.






16. 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






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






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






19. 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






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






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






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






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






26. 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.






27. 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.






28. 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.






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






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






32. The vapor pressure increases with increasing _____.






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






34. 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.






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






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






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






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






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

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






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






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






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






45. 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).






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

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






48. Electronegativities _______ as you go down a group.






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






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