A sample of oxygen gas contains 22.5 mol in a volume of 16.0 L. If the pressure and temperature are kept constant, but the volume is changed to 8.04 L, how

Question

many moles of oxygen gas does the sample contain? Be sure your answer has the correct number of significant figures.

Answer 1

To solve this problem, we can use the formula for the ideal gas law:
PV = nRT

Where:
P = pressure (constant)
V = volume
n = number of moles
R = ideal gas constant
T = temperature (constant)

Given:
Initial number of moles (n1) = 22.5 mol
Initial volume (V1) = 16.0 L
Final volume (V2) = 8.04 L

From the ideal gas law, we can set up the following equation:
P(V1) = n1RT
P(V2) = n2RT

Since the pressure and temperature are constant, we can equate the two equations:
V1/n1 = V2/n2
16.0 L / 22.5 mol = 8.04 L / n2

Solving for n2:
n2 = (8.04 L / 16.0 L) * 22.5 mol
n2 = 11.34 mol

Therefore, when the volume is changed to 8.04 L, the sample of oxygen gas contains 11.34 moles (rounded to three significant figures).