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

Step-by-step 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}=(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* 3.5L=0.5mol* 0.0821\text{ L. atm }mol^(-1)K^(-1)* 348K\\\\P=(0.5* 0.0821* 348)/(3.5)=4.08atm`

Hence, the pressure of CO gas is 4.08 atm