What volume do 3.8 x 10^22 molecules of NO2 gas occupy at STP?
1 mole will contain 6.022E23 molecules and occupy 22.4 L at STP. How many moles do you have?
3.8E22/6.022E23 = ??
?? moles x 22.4 L/mole = xx L.
To find the volume of a given number of gas molecules at STP (Standard Temperature and Pressure), we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
At STP, the pressure is 1 atmosphere (atm) and the temperature is 273.15 Kelvin (K). The ideal gas constant (R) is approximately 0.0821 L·atm/(mol·K).
First, let's calculate the number of moles of NO2 gas:
Number of molecules = 3.8 x 10^22
Avogadro's number (number of molecules per mole) = 6.022 x 10^23 molecules/mol
Number of moles (n) = Number of molecules / Avogadro's number
n = (3.8 x 10^22) / (6.022 x 10^23)
n ≈ 0.063 mol
Now, we have the number of moles (n), the pressure (P), the temperature (T), and the ideal gas constant (R). We can rearrange the ideal gas law equation to solve for the volume (V):
V = (nRT) / P
Substituting the values:
V = (0.063 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / 1 atm
V ≈ 1.65 L
Therefore, 3.8 x 10^22 molecules of NO2 gas occupy approximately 1.65 liters at STP.