how many molecules of CH4 gas are present in a 1.00 L flask of CH4 gas at STP?
How many moles are present? 1 mole will occupy 22.4 L and it will contain 6.022E23 molecules.
PV=nRT
1 atm *1.00L= n * 0.0821(atm-L/ mol-K) * 273 k
n= 0.0446 mol
0.0446 mol * 6.02 * 10^23 (molecules/mol)=
6.28* 10^22
1l contain =6.022×10^23/22.4
=2.68×10^22
To determine the number of molecules of CH4 gas in a 1.00 L flask at STP (Standard Temperature and Pressure), we need to use the ideal gas law and Avogadro's number.
Avogadro's number (NA) represents the number of molecules or atoms in one mole of any substance. Its value is approximately 6.022 x 10^23 molecules/mol.
STP is defined as a temperature of 273.15 K (0 degrees Celsius) and a pressure of 1 atm.
First, let's find the number of moles of CH4 gas using the ideal gas law:
PV = nRT
P: Pressure (1 atm)
V: Volume (1.00 L)
n: Number of moles (unknown)
R: Ideal Gas Constant (0.0821 L·atm/mol·K)
T: Temperature (273.15 K)
Rearranging the formula to solve for n:
n = PV / RT
n = (1 atm) * (1.00 L) / (0.0821 L·atm/mol·K * 273.15 K)
n ≈ 0.0447 mol
Now, to find the number of molecules, we multiply the number of moles by Avogadro's number:
Number of molecules = n * NA
Number of molecules = 0.0447 mol * (6.022 x 10^23 molecules/mol)
Number of molecules ≈ 2.69 x 10^22 molecules
Therefore, in a 1.00 L flask of CH4 gas at STP, there are approximately 2.69 x 10^22 molecules of CH4.