If you have 22.46 mLs of a gas at STP, how many moles of gas do you have?
22.46 mL x ( 1 mol/22,400 mL) = ? mols.
To find the number of moles of gas, we can use the ideal gas law, which is expressed as:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature
At STP (Standard Temperature and Pressure), the pressure is 1 atm (atmosphere) and the temperature is 273.15 K (Kelvin).
The gas constant, R, is a constant value that depends on the units of pressure, volume, and temperature used. The value of R is 0.0821 L·atm/(mol·K).
In this case, we have the volume (V) of the gas at STP, which is 22.46 mL. However, we need to convert it to liters (L) since the gas constant is given in liters.
To convert from milliliters (mL) to liters (L), we divide the volume by 1000:
V = 22.46 mL / 1000 = 0.02246 L
Now we can plug in the values into the ideal gas law equation:
(1 atm) * (0.02246 L) = n * (0.0821 L·atm/(mol·K)) * (273.15 K)
Simplifying the equation, we get:
0.02246 = n * 22.414
Solving for n, we divide both sides by 22.414:
n = 0.02246 / 22.414 ≈ 0.001 mol
Therefore, you have approximately 0.001 moles of gas.