Final answer:
The volume of 2.43 x 10^23 molecules of N2 gas at STP is 0.915 L.
Step-by-step explanation:
The volume of 2.43 x 1023 molecules of N2 gas at STP can be calculated using the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin. At STP, the pressure is 1 atm and the temperature is 273 K. Since we know the number of molecules (2.43 x 1023) and N is the same for all types of gases, we can calculate the number of moles of N2 gas.
Using Avogadro's number, which is 6.022 x 1023 molecules per mole, we can divide the number of molecules by Avogadro's number to get the number of moles. In this case, (2.43 x 1023) / (6.022 x 1023) = 0.0403 moles of N2 gas.
Now, we can use the ideal gas law to calculate the volume. Rearranging the equation, V = (nRT) / P, we can plug in the values: V = (0.0403 moles x 0.0821 L·atm/mol·K x 273 K) / 1 atm = 0.915 L.