Question

a gaseous mixture containing 0.35gm of N2 and 5600ml of O2 at s.t.p. is kept in a 5litres flask at 300K. the total pressure of the gaseous mixture is​

Answer 1

Answer: The total pressure of the gaseous mixture is 1.30 atm

Explanation:

• For nitrogen gas:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of nitrogen gas = 0.35 g

Molar mass of nitrogen gas = 28 g/mol

Putting values in above equation, we get:

$\text{Moles of nitrogen gas}=\frac{0.35g}{28g/mol}=0.0125mol$

• For oxygen gas:

According to mole concept:

22.4 L of 22400 mL of volume is occupied by 1 mole of a gas

So, 5600 mL of volume will be occupied by = $\frac{1}{22400}\times 5600=0.25mol$ of oxygen gas

To calculate the pressure of the mixture, we use ideal gas equation:

$PV=nRT$

where,

P = pressure of the mixture = ?

V = Volume of the mixture = 5 L

T = Temperature of the mixture = 300 K

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

n = Total number of moles = (0.0125 + 0.25) = 0.2625 moles

Putting values in above equation, we get:

$P\times 5L=0.2625mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 300K\\P=1.30atm$

Hence, the total pressure of the gaseous mixture is 1.30 atm

Answer 2

Answer:

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