If an 8-g sample of molecular oxygen at 1.00 atm pressure occupies 3.00 L, calculate the temperature of the sample.
A) 146°C
B) 146 K
C) 73°C
D) 73 K

Question

Quizplus · Accepted Answer

The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. We can solve for T by rearranging the equation: T = PV/nR.

First, we need to calculate the number of moles of oxygen in the sample. The molar mass of O2 is 32 g/mol, so 8 g of O2 is equivalent to 0.25 mol.

Next, we can plug in the values we have:

T = (1.00 atm)(3.00 L)/(0.25 mol)(0.08206 L·atm/mol·K)

Simplifying, we get:

T = 97.05 K

Converting to Celsius, we get approximately 146 K.

If an 8-G Sample of Molecular Oxygen at 1