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






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






3. The temperature at which a substance's solid and liquid phases are in equilibrium.






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






5. 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.






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






7. *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.






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






9. 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.






10. 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.






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






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






13. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.






14. Electronegativities _______ as you go down a group.






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






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 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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18. 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).






19. 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.






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






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






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






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






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






25. 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.






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






28. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.






29. 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






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






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






32. 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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33. 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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34. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.






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






36. 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.






37. 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 _____ _






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






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






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






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






43. **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.






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






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






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






47. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.






48. 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.






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






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