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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 relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).






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






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






4. *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.






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






6. 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.






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






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






9. Rays made up of positive electrodes in basic electron charges.






10. Electronegativities _______ as you go down a group.






11. 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.






12. The energy required to remove an electron from an isolated atom in its ground state.






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






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






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






16. 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.






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






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






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






20. 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.






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






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






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






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






25. 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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26. 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.






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






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

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29. 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.






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






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






32. **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.






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






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






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






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






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






38. 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






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






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






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






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






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






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






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






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






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






49. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.






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







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