Question

Suppose you have 0.100 m3 of CO2, at pressure of 2.00 atm, and a temperature of 30.0◦C. How many grams of CO2 do you have? Express your answer in grams.

Answer 1

Answer:- 354 g.

Solution:- It is a problem based on an ideal gas law equation, PV = nRT

Where P is pressure in atm, V is volume in liters, n is number of moles, R is the universal gas constant and T is kelvin temperature.

Value of R is 0.0821 atm.L per mol per kelvin.

P = 2.00 atm

T = 30.0 + 273 = 303 K

V = 0.100 cubic meter.

We need to convert the volume from cubic meter to liters.

1 cubic meter = 1000 L

So, $0.100m^3(\frac{1000L}{1m^3})$

= 100 L

Let's plug in the values in the equation and calculate the moles of the gas that could further be converted to grams on multiplying the moles by molar mass.

The rearranged equation for the moles, n is:

$n=\frac{PV}{RT}$

$n=\frac{2.00atm*100L}{\frac{0.0821atm.L}{mol.K}*303K}$

n = 8.04 moles

Molar mass of carbon dioxide is 44.01 g per mol. Let's multiply the moles by molar mass to get  the grams:

$8.04moles(\frac{44.01g}{mol})$

= 353.84 g

It could be round off to 354 g. So, the mass of the carbon dioxide gas we have is 354 g.