Question

What is the density (in g/L) of a gas with

a molar mass of 32.49 g/mol at
2.569 atm and 458 K?​

Answer 1

2.22 g/L

Step-by-step explanation:

Answer 2

2.22 g/L

Step-by-step explanation:

There's a relationship using the ideal gas law between molar mass and density:
`MM=(dRT)/(P)`, where MM is the molar mass, d is the density, R is the gas constant, T is the temperature, and P is the pressure.

We know from the problem that MM = 32.49 g/mol, T = 458 Kelvin, and P = 2.569 atm. The gas constant, R, in terms of the units atm and Kelvin is 0.08206. Let's substitute these values into the formula:

`MM=(dRT)/(P)`

`32.49g/mol=(d*0.08206*458K)/(2.569atm)`

Solve for d:

d * 0.08206 * 458 K = 32.49 * 2.569

d = (32.49 * 2.569) / (0.08206 * 458 K) ≈ 2.22 g/L

The answer is thus 2.22 g/L.

~ an aesthetics lover