Step-by-step explanation:
The theoretical volume of ammonia that should be produced in the Haber process if we start with 5.0 L of nitrogen (N2) at standard temperature and pressure (STP) can be calculated as follows:
1 mole of N2 reacts with 3 moles of H2 to form 2 moles of NH3
Thus, the number of moles of N2 present can be calculated using the Ideal Gas Law:
PV = nRT
Where n is the number of moles of gas, R is the gas constant, T is the temperature in Kelvin, P is the pressure in atmospheres, and V is the volume in liters.
At STP (0°C and 1 atm), the volume of one mole of gas is 24.45 L.
Given 5.0 L of N2 at STP, the number of moles of N2 can be calculated as:
n = (PV)/RT = (1 atm)(5.0 L)/(0.0821 atmL/molK)(273 K) = 1.96 moles
The number of moles of NH3 produced can then be calculated as:
n = (2 moles of NH3)/(1 mole of N2) = 2 moles/1 mole = 2 moles
The volume of NH3 can be calculated as:
V = nRT/P = (2 moles)(0.0821 atmL/molK)(273 K)/(1 atm) = 44.8 L
So, the theoretical volume of ammonia (NH3) that should be produced if we start with 5.0 L of N2 at STP is 44.8 L.