Help with gas law problems in chemistry?

At 27 ºC, the volume of a gas is 73.0 mL. At the same pressure, its volume is 272 mL at what temperature?

Select one:

a. 850

b. 1118.37

c. -170

d. -190

The volume of a gas is 610.7 mL at 28.2 ºC. If the temperature is increased to 60.8 ºC without changing the pressure, what is the new volume of the gas?

Select one:

a. 677

b. 551

c. 1320

d. 10.7

At 517 mm Hg, a sample of nitrogen gas occupies 870 mL. What volume does the gas occupy if the temperature remains constant and the pressure increases to 755.7 mm Hg?

Select one:

a. 595

b. 449

c. 0.00393

d. 1470

The pressure of a sample of helium is 6.890 atm in a 258.5 mL container. If the container is compressed to 32.9 mL without changing the temperature, what is the new pressure?

Select one:

a. 54.1

b. 0.877

c. 1230

d. 327

The volume of a gas collected when the temperature is 11.5 ºC and the pressure is 689.3 mm Hg measures 11.5 mL. What is the calculated volume of the gas at 44.7 ºC and 747.5 mm Hg?

Select one:

a. 31.5

b. 110

c. 37.1

d. 4.43

Update:

If anyone even understands one please help me even if you don't know all

1 Answer

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  • 5 months ago

    Every one of the 20 proposed answers here is wrong, because no units are shown.

    (27 + 273.15) K x (272 mL / 73.0 mL) = 1118.37 K

    [although no more than two significant digits are justified.]

    -----------------------

    (610.7 mL) x (60.8 + 273.15) K / (28.2 + 273.15) K = 677 K

    --------------------

    (870 mL) x (517 mm Hg / 755.7 mm Hg) = 595 mL

    ---------------------

    (6.890 atm) x (258.5 mL / 32.9 mL) = 54.1 atm

    ---------------------

    (11.5 mL) x (44.7 + 273.15) K / (11.5 + 273.15) K x (689.3 mm Hg / 747.5 mm Hg) = 11.8 mL

    [I'm guessing one of the two "11.5" values in the question got copied incorrectly.]

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