a sample of hydrogen gas has a volume of 15.0L AT 740 mm Hg. what will the volume at 800 mm H g?

Question

what will be the volume at 800 mm Hg, 700 torr and 2.0 atm?

Answer 1

At constant temperature, a closed ideal gas obeys the relation PV= constant.
15L x 740 mm = 11100 L-mm Hg.
(x) x 800 mm = 11100 L-mm Hg, so x = 11100/800 L
or 13.9 L
Torr is a unit of pressure 1 Torr=1 mm Hg, so we can solve:
(y) x 700 torr = 11100 L-torr, so x = 11100/700=15.6 L
Atm is a unit of pressure 1 atm=760 mm Hg. So 2 atm=
1620 mm Hg. Solve similar to above.

Answer 2

Since you didn't state all information, I will make the assumption that the gas is in a fixed enclosure. Thus, the answer is 15.0L .

The temperature of the (ideal) H2 gas in a 15.0L container will vary, depending on pressure and molecular quantity (moles) of H2 is the volume:

740 mmHg = T1
800 mmHg = 740/800 x T1
2.0 atm = 740/1520 x T1
700 torr = 740/700 x T1

If you assume the gas is at room temperature (290 degrees Kelvin), the volume is then calculated according to the same ratios, yielding a volume at 700 torr of 15.86L
(15 x 740/700).

Answer 3

This is a Boyle's Law problem:

P1V1 = P2V2

P1 = 740 mmHg
V1 = 15.0 L
P2 = 800 mmHg
V2 = ?

Rearrange your formula so V2 is on the side by itsself:

V2 = P1V1 / P2

Plug in your values, cancel units that are the same in both numerator and denominator, and then do the math.

V2 = (740 mmHg)(15.0 L) / (800 mmHg)

mmHg cancel leaving your units L

V2 = 13.88 L

Always look at the values you are given. Chose the gas law with those variables. Write your formula for the gas law. Set up your table of values so you keep beginning and ending values straight. Rearrange your formula so what you want is isolated. THEN, plug in the values you have and solve for the unknown. All units should cancel except for the units you are looking for. If you get any other units when cancelling, then you set your problem up incorrectly.

To solve the problem so you get your answer in Torr, you need to convert your beginning pressure to Torr:

1 Torr = 1 mmHg

To solve the probem so you get your answer in atm, you need to convert your beginning pressure to atm:

1 atm = 760 mmHg

(as you can see, 1atm = 760 mmHg = 760 Torr)

Your beginning and ending pressures need to be in the same unit to work the problem.

CHEMISTRY TEACHER

Answer 4

comvert to L
divide
multiply to get volume at 800 mm Hg, 700 torr and 2.0 atm

Answer 5

Your gas is measured at a stress diverse than widely used stress (a million.0 surroundings), so that you should correct ideal the volume for this. Your gas is likewise measured at a temperature diverse than widely used temperature (273 ok) so that you should correct ideal the volume for this. in case you combine Boyle's regulation (mandatory for the stress correction) and Charles' regulation (mandatory for the temperature correction) you'll probable use the formula: P1V1/T1 = P2V2/T2 P1, V1, T1 are your unique numbers (do now no longer ignore about to regulate celcius to kelvin with the help of which includes 273). P2 is your widely used stress, a million.0 atm T2 is your widely used temperature, 273 ok V2 is your unknown. Plug contained in the numbers and chug out an answer.