what volume does 3.01x 10^21 molecules of N2 occupy at STP
1 mol of a gas at STP occupies 22.4L and contains 6.02E23 molecules.
Convert 3.01E21 molecules to moles and that to L.
To determine the volume occupied by a given number of molecules of a gas at STP (Standard Temperature and Pressure), you can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in Pascals (Pa)
V = volume in cubic meters (m^3)
n = number of moles of gas
R = ideal gas constant (8.314 J/(mol·K))
T = temperature in Kelvin (K)
In this case, you need to find the volume, so we rearrange the equation to solve for V:
V = (nRT) / P
First, let's calculate the number of moles (n) of N2:
Given number of molecules of N2 = 3.01 x 10^21
Avogadro's number (number of molecules in one mole) = 6.022 x 10^23
n = (Number of molecules) / (Avogadro's number)
n = (3.01 x 10^21) / (6.022 x 10^23)
n ≈ 0.04997 moles
Next, we substitute the known values into the equation and solve for V:
P = standard pressure at STP = 1 atmosphere = 101,325 Pascals
T = standard temperature at STP = 273.15 Kelvin
V = (nRT) / P
V = (0.04997 moles) * (8.314 J/(mol·K)) * (273.15 K) / 101325 Pa
After the calculations, you will have the volume in cubic meters.