What volume would 1.5 x 10^25 molecule CO2 occupy at STP?
To find the volume, we need to 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 (Standard Temperature and Pressure), the values are typically P = 1 atm and T = 273.15 K.
First, we need to determine the number of moles of CO2. We can use Avogadro's number to convert the number of molecules to moles. Avogadro's number is 6.022 x 10^23 molecules/mole.
So, 1.5 x 10^25 CO2 molecules = (1.5 x 10^25 molecules) / (6.022 x 10^23 molecules/mole) = 24.928 moles.
We also have to note that CO2 is a gas at STP, so the gas constant R is 0.0821 L·atm/(mol·K).
Next, we can plug the values into the ideal gas law equation:
PV = nRT
We know P = 1 atm, n = 24.928 moles, R = 0.0821 L·atm/(mol·K), and T = 273.15 K.
Solving for V, we get:
V = (nRT) / P
= (24.928 mol) x (0.0821 L·atm/(mol·K)) x (273.15 K) / (1 atm)
= 627.4 L
Therefore, 1.5 x 10^25 CO2 molecules would occupy 627.4 liters of volume at STP.
moles= 1.5E23/avagnumber
volume= 22.4 dm^3 * number of moles.