Answer:
χH₂ = 0.4946
χN₂ = 0.4130
χAr = 0.0923
Explanation:
The total pressure of the mixture (P) is:
P = pH₂ + pN₂ + pAr
P = 443.0 Torr + 369.9 Torr + 82.7 Torr
P = 895.6 Torr
We can find the mole fraction of each gas (χ) using the following expression.
χi = pi / P
χH₂ = pH₂ / P = 443.0 Torr/895.6 Torr = 0.4946
χN₂ = pN₂ / P = 369.9 Torr/895.6 Torr = 0.4130
χAr = pAr / P = 82.7 Torr/895.6 Torr = 0.0923
Atoms like in chemistry class?
Answer:
1.52atm is the pressure of the gas
Explanation:
To solve this question we must use the general gas law:
PV = nRT
<em>Where P is pressure in atm = Our incognite</em>
<em>V is volume = 50.5L</em>
<em>n are moles of gas = 3.25moles</em>
<em>R is gas constat = 0.082atmL/molK</em>
<em>And T is absolute temperature = 288.6K</em>
To solve pressure:
P = nRT / V
P = 3.25mol*0.082atmL/molK*288.6K / 50.5L
P = 1.52atm is the pressure of the gas
The density of CO2 getting from experiment is 0.1/0.056 = 1.79 g/L. The percent error of this is (1.96 -1.79)/1.96*100%=8.67%. So the approximate percent error is 8.67%.
