A sample of gas exhibits ideal behavior and occupies a volume of 350 mL at 25.0 C and 1.00atm. How many moles of gas are present in the sample?
P V = n R T
so
n = PV / RT
T = 25 +273 = 298 degrees Kelvin
P= 1 atm = 1.013*10^5 Pascals
V = 0.350 Liters
R = 8.315 J/mol deg K
so
n = 1.013 * 10^5 * 0.350 / ( 8.315 * 298) = 14.3 mol
sorry, V should be in meters^3 with that R value
and we can use1 atm if we use
R = 0.08206 L atm / mol*deg K
n = 1 atm * 0.350 Liters / 0.08206*298 = 0.0143 mols
To find the number of moles of gas present in the sample, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)
First, we need to convert the given values to the correct units:
Volume = 350 mL = 350/1000 L = 0.35 L
Temperature = 25.0 C = 25.0 + 273.15 K = 298.15 K
Pressure = 1.00 atm
Now, we can plug these values into the ideal gas law equation to solve for the number of moles:
PV = nRT
1.00 atm * 0.35 L = n * 0.0821 L.atm/mol.K * 298.15 K
0.35 = 0.0821 * 298.15 * n
n = 0.35 / (0.0821 * 298.15)
n = 0.0146 moles
Therefore, there are approximately 0.0146 moles of gas present in the sample.