Problems. To receive full credit, you must show all your work (Gas Law Constamt

Question

Problems. To receive full credit, you must show all your work (Gas Law Constamt R-00821 atm/mol K OR 62.4 L torr/mol K) 1. (10 points) A sample of nitrogen gas occupies a volume of 8 50 L. at 0.980 atm. What volume does the gas occupy if the pressure is increased to 1.30 atm? 2. (10 points) A helium sample at 25 C has a volume of 1.82 L. If the pressure and amount of helium remain unchanged what will the volume of the gas be at 50°C? (10 points) A 0.85 mol of a gas has a volume of 758 Torr and a volume of 21.0L. What will the volume be if the amount is increased to 1.00 mol and the pressure remains 3. unchanged?

Explanation / Answer

ANSWER #1

Using the Boyle's Law:

P1V1 = P2V2 (1)

We have the initial conditions: P1 = 0.980 atm, and V1 = 8.50 L

For a final pressure of: P2 = 1.30 atm

We must rearrange the equation (1) to calculate the final volume of the gas (V2):

V2 = (P1/P2)V1

Substituting known data:

V2 = (0.980 atm / 1.30 atm) * 8.50 L = 6.41 L

THE VOLUME THAT THE GAS OCCUPIES IF PRESSURE IS INCREASED TO 1.30 atm IS 6.41 L

ANSWER #2

Using the Charles's Law:

(T1/V1) = (T2/V2) (2)

We have the initial conditions: T1 = 25ºC, and V1 = 1.82 L

For a final temperature of: T2 = 50ºC

We must rearrange the equation (2) to calculate the final volume of the gas (V2):

(T2/T1)V1 = V2

Also, we need convert the temperature given to the Kelvin scale, as follows:

T1 = 25ºC +273 = 298 K

T2 = 50ºC +273 = 323 K

Substituting known data:

(323 K / 298 K) * 1.82 L = 1.97 L

THE FINAL VOLUME OF THE HELIUM AT 50ºC WILL BE 1.97 L

ANSWER #3

Using the Avogadro's hipothesys:

(n1/V1) = (n2/V2) (3)

We have the initial conditions: n1 = 0.85 mol, and V1 = 21.0 L

For a final amount of substance of: n2 = 1.00 mol

We must rearrange the equation (3) to calculate the final volume of the gas (V2):

(n2/n1)V1 = V2

Substituting known data:

(1.00 mol / 0.85 mol) * 21.0 L = 24.7 L

THE FINAL VOLUME OF THE GAS IS 24.7 L

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