Question

How many grams of sulfur dioxide (SO2) are there in a 3.50 L container at 100°C and a pressure of 2.00 atm?

Answer 1

Answer: The mass of sulfur dioxide is 14.6 grams

Step-by-step explanation:

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

`PV=nRT`

where,

P = pressure of the sulfur dioxide = 2.00 atm

V = Volume of the sulfur dioxide = 3.50 L

T = Temperature of the mixture =
`100^oC=[100+273]K=373K`

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

n = number of moles of sulfur dioxide = ?

Putting values in above equation, we get:

`2.00atm* 3.50L=n_(SO_2)* 0.0821\text{ L atm }mol^(-1)K^(-1)* 373K\\\\n_(SO_2)=(2.00* 3.50)/(0.0821* 373)=0.228mol`

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

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

Moles of sulfur dioxide = 0.228 moles

Molar mass of sulfur dioxide = 64 g/mol

Putting values in above equation, we get:

`0.228mol=\frac{\text{Mass of sulfur dioxide}}{64g/mol}\\\\\text{Mass of sulfur dioxide}=(0.228mol* 64g/mol)=14.6g`

Hence, the mass of sulfur dioxide is 14.6 grams