Answer:
5 moles of Argon is present in the mixture.
Explanation:
Total pressure of the gaseous mixture = 4 atm
Total number of moles = 16
Partial pressure of Ne = 2.75 atm
By Dalton's law of partial pressure, the total pressure of gaseous mixture is the sum of partial pressures of individual gases which are non-reactive.
Hence:
Also :
Partial pressure = mole fraction*total pressure
∴Number of moles of Argon = 5
Answer:
1711.11L
Explanation:
Given parameters:
Mass of methane = 1kg = 1000
Temperature of gas = 35°C
Pressure of the gas = 0.9atm
Converting to the temperature to kelvin, we have:
35+ 273 = 308k
Solution
From the given parameters, we can solve this problem using the ideal gas equation which is combination of the gas laws. It is expressed below:
PV = nRT .......................(i)
Where P is the pressure of the gas
V is the volume of the gas
n is the number of moles
R is the gas constant
T is the temperature
Now, from the above parameters, we have two unknowns which are n and V.
To find the number of moles n, we use the expression below:
number of moles =
molar mass of methane = 12 + (4x1) = 16g/mol
Number of moels of methane = = 62.5mole
Now that we know the number of moles, we can make the unknown Volume the subject of the formula:
V =
V = = 1711.11L