Answer:
1.46 mol of H₂
Explanation:
This easy question can be solved by a rule of three.
At STP conditions, we know that 1 mol of any gas is contained in 22.4L.
So let's make the operation:
22.4L is the volume for 1 mol of any gas, at STP
32.6 L may be the volume for (32.6 . 1) /22.4 = 1.46 moles.
We can also apply, the Ideal Gases Law.
At STP conditions, Temperature is 273.15 K and pressure is 1 atm
P . V = n . R . T
n = (P . V) / R. T → (1 atm . 32.6L) / (0.082 . 273.15K)
n = 1.455 mol
