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






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






3. 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.






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






5. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.






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






7. 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






8. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.






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






10. 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.






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






12. *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.






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






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






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






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






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






18. *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






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






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






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






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






23. 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.






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






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






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






28. _____ bonds are present in molecules containing double or triple bonds.






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






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






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. 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.






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






34. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.






35. A hypothetical gas would follow Boyles law under all conditions and is called?






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






37. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.






38. 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.






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






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






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






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






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






45. 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






46. 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.






47. 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.






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






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






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







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