A 1.50 liter flask at a temperature of 25°C contains a mixture of 0.158 moles of methane, 0.09 moles of ethane, and 0.044 moles of butane. What is the total pressure of the mixture inside the flask?

The total amount of moles inside the flask is
n = 0.158 + 0.09 + 0.044 = 0.292 mole

According to Boyle's Law, the total pressure of a mixture in a container does not depend on the identity of the gas and only on the amount of the number of moles. So, assuming the mixture behaves like an ideas gas:
P = nRT/V = 0.292 (0.08206) (25+273) / (1.50)
P = 4.76 atm

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Anonymous Anonymous · Answer 2 · 2019-11-01T01:46:16-04:00

Answer: The pressure of the mixture inside the flask is 4.76 atm

Explanation:

To calculate the pressure, we use the equation given by ideal gas equation:

PV = nRT

where,

P = Pressure of the flask = ?

V = Volume of the flask = 1.50 L

n = Total number of moles = 0.158 + 0.09 + 0.044 = 0.292 moles

R = Gas constant = \(0.0820\text{ L atm }mol^{-1}K^{-1}\)

T = Temperature of the flask = \(25^oC=[25+273]K=298K\)

Putting values in above equation, we get:

\(P\times 1.50L=0.292mol\times 0.0820\text{ L atm }mol^{-1}K^{-1}\times 298K\\\\P=\frac{0.292\times 0.0820\times 298}{1.50}=4.76atm\)

Hence, the pressure of the mixture inside the flask is 4.76 atm