How many moles of N2 can be in a balloon with a volume of 6.00 L at STP?
You should remember that 1 mole of N2 will occupy a volume of 22.4L at STP.
To determine the number of moles of N2 in a balloon with a volume of 6.00 L at Standard Temperature and Pressure (STP), we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (STP is 1 atmosphere)
V = Volume (given as 6.00 L)
n = Number of moles (what we want to find)
R = Gas constant (0.0821 L·atm/mol·K)
T = Temperature (STP is 273.15 K)
Rearranging the equation, we get:
n = PV / RT
Plugging in the known values:
n = (1 atm) * (6.00 L) / (0.0821 L·atm/mol·K) * (273.15 K)
Simplifying:
n = 0.246 moles
Therefore, there can be approximately 0.246 moles of N2 in a balloon with a volume of 6.00 L at STP.