What is the partial pressure (in atm) of Krypton gas of gases if the mole fracti

Question

What is the partial pressure (in atm) of Krypton gas of gases if the mole fraction of Krypton is 0.35 and the total pressure of the mixture is 37 atm? How many moles are there in a sample of gas that occupies 9.06 L at 341.92 K and3.7 atm? What is the Volume (in mL)of a sample of gas at 1.6 atm. 329.43 K and 100.88 mL if the pressure is changed to 0.96 atm and the temperature is changed to 288 55 K? Place the following gases in order of rate of effusion with the highest rate of effusion first (highest effusion rate is number 1 to lowest effusion rate which will be number 4)

Explanation / Answer

1. Partial Pressure of Kr = Mole fraction of Kr * Total Pressure

= 0.35 * 3.7 = 1.295 atm ~ 1.3 atm

2. According to the ideal gas law

PV = n R T

P = 3.7 atm, V = 9,06 L , T = 341.92 K, R = 0.08206 L atm / mol K, n = moles = ?

Substituting the values in above equation,

n = PV / R T = 3.7 * 9.06 / ( 0.08206 * 341.92)

n = 1.1947 ~ 1.2 moles

3. Combining Boyle/Charles/Gay-Lussac law as follows:

P1 V1 / T1 = P2 V2 / T2........(a)

P1 = 1.6 atm , V1 = 100.88 mL , T1 = 329.43 K, P2 = 0.96 atm, T2 = 288.55 K, V2 = ?

Substituting all the above values in above equation (a)

(1.6 * 100.88) / 329.43 = (0.96 * V2) / 288.55

(1.6 * 100.88 * 288.55) / (329.43 * 0.96) = V2

V2 = 147.269 ~ 147.3

4. Efussion rate is basically the grahams law. rate which equals 1/weight. This means the biggest molecular weight the diatomic gas has, the smallest will be the effusion speed and the smallest molecular weight diatomic gas has the biggest (the fastest) effusion speed.

So the order of effusion is as follows:

1. H2

2. N2

3. F2

4. O2

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