A 1.0 liter flask is filled with a mixture of two gases at 20. oC until a pressure of 14.43 atm is established. If 0.40 grams of the mixture is hydrogen, how many moles are there of the other gases?
pv=nRT solve for n, total moles, then subtract the moles of hydrogen present.
.20mol
To find the number of moles of the other gases in the mixture, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature in Kelvin
First, let's convert the given temperature from 20.0 oC to Kelvin by adding 273.15:
T = 20.0 oC + 273.15 = 293.15 K
Now, we'll rearrange the ideal gas law equation to solve for the number of moles (n) of the other gases:
n = PV / RT
We already have the values for pressure (P) as 14.43 atm and volume (V) as 1.0 liter. The ideal gas constant (R) is 0.0821 L·atm/(mol·K).
Substituting the values into the equation:
n = (14.43 atm) * (1.0 L) / (0.0821 L·atm/(mol·K) * 293.15 K)
Now, we can calculate the number of moles (n) of the other gases by performing the calculation:
n = (14.43) / (0.0821 * 293.15)
n ≈ 0.647 mol
Therefore, there are approximately 0.647 moles of the other gases in the mixture.