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






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. *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.






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






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






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






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






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






9. 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).






10. 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.






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






12. *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






13. The freezing point is always lowered by addition of solute.






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






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






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






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






18. Cells that convert electrical energy into chemical energy.






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






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






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






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






23. 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.






24. 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.






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






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






27. 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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28. 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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29. 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






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






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






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






33. 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).






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






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






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






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






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






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






40. **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.






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






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






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






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






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






46. 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.






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






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






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

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