11.1 How many moles of gas are found in a 1000 dm3 container if the conditions inside the container are 298.15K and 2 atm?

Solution: Insert following values in proper fields: P = 2 atm, T = 298.15 K, V = 1000 dm3 and press Enter.

11.2 What volume will 120 grams of chlorine gas occupy at STP?

Solution:

First, find moles(n) by the use the molecular calculator and argument the Cl2 by 120g --> 120gCl2

Second, insert the STP values in proper fields (P,n,T) and press Enter.

11.3A steel tank contains 15.0 g of Cl2 gas under a pressure of 5.0 atm at 22.0 oC. What is the volume of the tank?

Solution:

First, use the units convertor to convert 22 oC to Kelvin.

Second, find (n) by inserting 15gCl2 in the molecular calculator and calculate.

Third, calculate V by inserting the values of P ,n and T in the Ideal Gas Law Calculator.

11.4 A balloon (100 g) was at sea level (1atm and 290K) filled with 1000 dm3 of hydrogen gas. Knowing that air contain approx. 21% oxygen, 78% nitrogen and 1% argon, how many grams was this balloon able to lift?.

Solution:

1) Calculate the mass of 1000 dm3 air:

78% of 1000 dm3 =780 dm3 of N2 gas.

Insert following values in the Ideal Gas Calculator:

V=790 dm3, P=1atm, T=290K and press Enter.

multiply the result (n) by 28g/mol and find the N2 mass in the balloon.

Use the same procedure as over, but this time for calculating the masses of O2 and argon.

2) The mass of 1000 dm3 air is obtained by adding mN2, mO2 and argon.

3)Calculate the mass of 1000 dm3 H2 (V=1000 ,P=1atm T=290K) Multiply the result (n) in this calculation by 2g/mol.

4) Result: mN2 + mO2 + mAr - 100g - mH2 = lift

Combined Gas Law

11.5 A gas was confined in a cylinder fitted with a movable piston. At 290K, the gas occupied a volume of 8.0 dm3 under a pressure of 1.85 atm. The gas was simultaneously heated and compressed, so that its volume was 6.45 dm3 and its temperature was 350K. What pressure was exerted by the hot compressed gas?

Solution:

Insert following values in proper fields: T1 = 290 K, V1 = 8.00 dm3, P1 = 1.85 atm, T2 = 350 K, V2 = 6.45 dm3 and press Enter.

Graham's Law of Diffusion

11.6 What is the ratio of the velocity of helium atoms to the velocity of radon atoms (v1 to v2) when both gases are at the same temperature? Mass: Radon=222 u, Helium=4.00 u

Solution:

Insert 222 in the m2 field, 4 in the m1 field and 1 in the v2 field. The v1/v2 ratio will be calculated by pressing Enter.

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