If you have 4.90 moles of Ba, how many liters of N2 would you have at STP?
I wouldn't have any N2 unless someone slipped some in while I wasn't looking.
To determine the number of liters of N2 at STP (Standard Temperature and Pressure), you can use the concept of molar volume.
Molar volume is the volume occupied by one mole of a gas at STP, which is defined as 22.4 liters per mole.
Given:
Moles of Ba = 4.90 moles
Since Ba and N2 have a 1:1 stoichiometric ratio in the balanced equation, it means that for every mole of Ba, there is one mole of N2 produced.
Therefore, the number of moles of N2 would also be 4.90 moles.
To find the volume occupied by 4.90 moles of N2, we can use the molar volume:
Volume of N2 = Moles of N2 * Molar Volume
= 4.90 moles * 22.4 L/mole
= 109.76 liters
So, if you have 4.90 moles of Ba, you would have 109.76 liters of N2 at STP.