Question

Dry ice is solid carbon dioxide. A 1.65−g sample of dry ice is placed in an evacuated 3.93−L vessel at 23.0°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.

Answer 1

Answer: The pressure of the gas inside the vessel is 0.232 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 carbon dioxide = 1.65 g

Molar mass of carbon dioxide = 44 g/mol

Putting values in above equation, we get:

`\text{Moles of carbon dioxide}=(1.65g)/(44g/mol)=0.0375mol`

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 = 3.93 L

T = Temperature of the gas =
`23^oC=[23+273]=296K`

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

n = number of moles of gas = 0.0375 moles

Putting values in above equation, we get:

`P* 3.93L=0.0375mol* 0.0821\text{ L. atm }mol^(-1)K^(-1)* 296K\\\\P=(0.0375* 0.0821* 296)/(3.93)=0.232atm`

Hence, the pressure of the gas inside the vessel is 0.232 atm