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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 _____ 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.






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






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






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






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






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






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






8. 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.






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






10. 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.






11. The vapor pressure increases with increasing _____.






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






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






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






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






16. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.






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






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






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






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






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






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






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






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






25. 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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26. Metals have electronegativities less than ____






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






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






30. 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.






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

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






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






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






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






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






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

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






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






40. 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.






41. 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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42. 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.






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






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






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






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






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






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






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






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






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