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[answered] A gas is considered "ideal" if on

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1. A gas is considered "ideal" if one mole of it in a one-liter container exerts a pressure of exactly 1 atm at


room temperature.


a. True


b. False


2. The density of HCN is ________ g/L at STP.


a. 1.21


b. 329


c. 605


d. 0.829


e. 2.21


3. The volume of 1.26 mol of gas at 69.4 kPa and 25.30 ?C is ________ L.


a. 45.1


b. 633


c. 3.82


d. 0.445


e. 0.439


4. A helium balloon is filled to a volume of 27.7 L at 300 K. What will the volume of the balloon become if


the balloon is heated to raise the temperature to 392 K?


a. 36.2


b. 21.2


c. 0.0276


d. 0.0472


e. 3,260,000


5. A balloon originally had a volume of 4.39 L at 44 ?C and a pressure of 729 torr. The balloon must be


cooled to ________ ?C to reduce its volume to 3.99 L (at constant pressure).


a. 0.00


b. 15.1


c. -288


d. 288


e. 546


6. Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation:


2NaN3 (s) ? 2Na (s) + 3N2 (g).


What mass (g) of NaN3 is required to provide 26.5 L of N2 at 22.0 ?C and 1.10 atm?


a. 52.2


b. 700.


c. 0.807


d. 1.21


e. 1.10


7. Which statement about atmospheric pressure is false?


a. As air becomes thinner, its density decreases.


b. Air actually has weight.


c. With an increase in altitude, atmospheric pressure increases as well.


d. The warmer the air, the lower the atmospheric pressure.


e. Atmospheric pressure prevents water in lakes, rivers, and oceans from boiling away.


8. The pressure exerted by a column of liquid is equal to the product of the height of the column times the


gravitational constant times the density of the liquid, P = ghd. How high a column of water (d = 1.0 g/mL)


would be supported by a pressure that supports a 713 mm column of mercury (d = 13.6 g/mL)?


a. 14 mm b. 52 mm


c. 713 mm


d. 1.2 x 104 mm


e. 9.7 x 103 mm


9. One significant difference between gases and liquids is that ________.


a. A gas is made up of molecules


b. A gas expands to fill its container


c. A gas may consist of both elements and compounds


d. Gases are always mixtures


e. All of the above answers are correct.


10. As a gaseous element condenses, the atoms become ________ and they have ________ attraction for


one another.


a. more separated, more


b. more separated, less


c. closer together, more


d. closer together, less


e. larger, greater


11. The phase diagram of a substance is given below. This substance is a ________ at 30 ?C and 0.5 atm. a. Liquid


b. Gas


c. Solid


d. Supercritical fluid


e. Crystal


12. Ethanol (C2H5OH) melts at -114 ?C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and


liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g


of solid ethanol at -135 ?C to liquid ethanol at -60 ?C?


a. 207.3


b. -13.3


c. 6.34


d. 3617


e. 8.63


13. Of the following substances, ________ has the highest boiling point.






c. C4H10


d. N2


e. Cl2 14. On the phase diagram shown below, segment ________ corresponds to the conditions of temperature


and pressure under which the solid and the gas of the substance are in equilibrium. a. AB


b. AC


c. AD


d. CD


e. BC


15. Based on molecular mass and dipole moment of the five compounds in the table below, which should


have the highest boiling point? a. CH3CH2CH3


b. CH3OCH3


c. CH3Cl




e. CH3CN


16. For a given substance that exhibits liquid-crystalline properties, the transition from solid to liquid-crystal


state occurs ________.


a. Over a range of temperatures between the melting point of the solid and the boiling point of the




b. At the melting point of the solid


c. Over a range of temperatures that includes the melting point of the solid


d. At a well-defined temperature above the melting point of the solid


e. At a well-defined temperature below the melting point of the solid


17. The predominant intermolecular force in CaBr2 is ________.


a. London-dispersion forces


b. Ion-dipole forces


c. Ionic bonding


d. Dipole-dipole forces


e. Hydrogen bonding 18. At elevated temperatures, nitrogen dioxide decomposes to nitrogen oxide and oxygen: NO2 (g) ? NO (g) + O2 (g) The reaction is second order in NO2 with a rate constant of 0.543 M-1s-1at 300 ?C. If the


initial [NO2] is 0.260 M, it will take ________ s for the concentration to drop to 0.075 M. a. 3.34


b. 0.0880


c. 2.29


d. 0.299


e. 17.5


19. A compound decomposes by a first-order process. If 13% of the compound decomposes in 60 minutes,


the half-life of the compound is ________.


a. 299


b. 20


c. 12


d. -18


e. -5


20. The reaction shown below is ________, and it is a ________ elementary reaction.


A + B + C ? ABC a. termolecular, rare


b. termolecular, common


c. unimolecular, common


d. bimolecular, rare


e. unimolecular, rare


21. A second-order reaction has a half-life of 12 s when the initial concentration of reactant is 0.98 M. The


rate constant for this reaction is ________ M -1s-1.


a. 12


b. 2.0 ? 10-2


c. 8.5 ? 10-2


d. 4.3 ? 10-2


e. 4.3


22. The kinetics of the reaction below were studied and it was determined that the reaction


rate increased by a factor of 9 when the concentration of B was tripled. The reaction is


________ order in B.


A + B ? P a.








e. Zero








One-half 23. The rate constant for a particular second-order reaction is 0.47 M -1s-1. If the initial concentration of


reactant is 0.25 mol/L, it takes ________ s for the concentration to decrease to 0.20 mol/L.


a. 2.1


b. 1.4


c. 1.0


d. 0.47


e. 0.20


24. Under constant conditions, the half-life of a first-order reaction ________. a. is the time necessary for the reactant concentration to drop to half its original value


b. is constant


c. can be calculated from the reaction rate constant


d. does not depend on the initial reactant concentration


e. All of the above are correct


25. In general, as temperature goes up, reaction rate ________.


a. goes up if the reaction is exothermic


b. goes up if the reaction is endothermic


c. goes up regardless of whether the reaction is exothermic or endothermic


d. stays the same regardless of whether the reaction is exothermic or endothermic


e. stays the same if the reaction is first order


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