Asample of 88.0 g co2 is held at 291 k in a 40.0 l container. what is the pressure this gas exerts on the container. express your answer in kpa.

- 121 kPa.

Solution:- mass, temperature and volume are given for carbon dioxide gas asked to calculate the pressure this gas exerts on the container.

It is based on ideal gas law equation, PV = nRT .

Where, P is the pressure in atm, V is the volume in Liters, n is the number of moles of the gas, R is the universal gas constant and it's value is and T is the kelvin temperature.

Given data:- mass = 88.0 g

T = 291 K

V = 40.0 L

P = ?

We need to convert the mass to moles and for this we divide the mass by molar mass. Molar mass of carbon dioxide gas is 44.01 gram per mol.

n = 2.00 mol

The equation could be rearranged for pressure as:

Let's plug in the values and solve this for P.

P = 1.1946 atm

Since the answer is asked to report in kPa, let's convert atm to kPa.

1 atm = 101.325 kPa

So,

= 121 kPa

So, the pressure this gas exerts on the container is 121 kPa.