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.

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.