Suppose that the pressure of 1.00 L if has is 380 mm Hg when the temperature is 200 K. At what temperature is the volume 200 L and the pressure 0.750 ATM?

Answer 1

This question is screaming at you to use the ideal gas law.

PV=nRT

(Pressure)(Volume)=(moles)(Gas Constant)(Temperature)

You can assume that there is 1 mole of gas. You can also assume there is 1atm of pressure for the first equation, and 2atm for the second, because the pressure is doubled. Just make sure you use the right gas constant.

So just plug in your numbers!

(2atm)(V)=(1mol)(.0821 L atm/mol K)(200K)

= 8.21L

Answer 2

For this problem, we will use Charles's Law, which states that the proportion of volume to temperature in a gaseous system remains constant given that the pressure remains constant:

Vinitial/Tinitial=Vfinal/Tfinal

Remember: this only works because the pressure is being held constant.

Also, a caveat before we continue: temperature must always be in units of degrees Kelvin (K)

First, we must convert the temperatures given in degrees Celsius to degrees Kelvin. This is easy to do, simply add 273 to the Celsius values:

Tinitial=25 deg C=(25+273) K=298 K

Tfinal= 80 deg C=(80+273) K=353 K

Now, by plugging all known values in Charles's Law, we get:

(40.0 L)/(298 K)=(Vfinal)/(353 K)

Vfinal=((40.0)(353))/(298)

Vfinal=47.3826

According to the rules of significant figures, we can only have three significant figures in our answer, so in the end, the final answer is:

Vfinal=47.4 L

Answer 3

Solution guide:

Transform temperature unit to Kelvin (40 C --> 313.15 K. Temperature using in ideal gas law is in absolute scale. It is also suggest to use Pressure in Pascal and Volume in m3 but not necessary.

Re arrange ideal gas law PV = nRT -> PV/RT = n = constant long as no additional mass

so

P1V1/T1 = P2V2/T2 if P constant then P1 = P2

V2 =V2T2/T1

Just solve you equation.

Answer 4

600.0ml convert to liters

(0.6L)(8.00atm)=(2.00atm)(V2)

DIVIDE: 4.8/2.00

V2= 2.4

Answer 5

800 atm

Answer 6

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Answer 7

800