Dinitrogen oxide, N2O, which is used in dentistry, is an anesthetic also called laughing gas. What is the pressure, in atmospheres, of 0.35 mol of N2O at 22 degrees Celsius in a 5.0 L container?

Considering the ideal gas law, the pressure of 0.35 mol of N₂O at 22 degrees Celsius in a 5.0 L container is 1.6933 atm.

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:  

P×V = n×R×T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances.

In this case, you know:

Replacing in the ideal gas law:

P× 5 L= 0.35 mol× 0.082× 295 K

Solving:

P= (0.35 mol× 0.082× 295 K)÷ 5 L

P=1.6933 atm

Finally, the pressure of 0.35 mol of N₂O at 22 degrees Celsius in a 5.0 L container is 1.6933 atm.

Learn more:

1.69 atm is the value for the pressure

Explanation:

Let's apply the Ideal Gases Law for this situation

P . V = n . R . T

Let's convert the T° from °C to K → T°C + 273 → 22°C + 273 = 295K

P = ( n. R. T) / V → (0.35 mol . 0.082L.atm / mol.K . 295K) / 5L = 1.69 atm

its mg hope this

chemistry sucks a**

explanation: