Question

What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C

Answer 1

Answer: The pressure of CO gas is 4.08 atm

Explanation:

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

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

Given mass of CO = 14 g

Molar mass of CO = 28 g/mol

Putting values in above equation, we get:

$\text{Moles of CO}=\frac{14g}{28g/mol}=0.5mol$

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

$PV=nRT$

where,

P = pressure of the gas = ?

V = Volume of the gas = 3.5 L

T = Temperature of the gas = $75^oC=[75+273]K=348K$

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

n = number of moles of CO gas = 0.5 moles

Putting values in above equation, we get:

$P\times 3.5L=0.5mol\times 0.0821\text{ L. atm }mol^{-1}K^{-1}\times 348K\\\\P=\frac{0.5\times 0.0821\times 348}{3.5}=4.08atm$

Hence, the pressure of CO gas is 4.08 atm