To determine the volume of NH3 produced when 2 liters of N2 gas is mixed with H2 gas at constant temperature and pressure, we need to consider the balanced chemical equation for the reaction between N2 and H2 to form NH3:
N2 + 3H2 -> 2NH3
According to the balanced equation, one molecule of N2 reacts with three molecules of H2 to produce two molecules of NH3. Therefore, the molar ratio between N2 and NH3 is 1:2.
Given that the initial volume of N2 is 2 liters, we can assume that it is measured at the same temperature and pressure as the resulting NH3. Using the ideal gas law (PV = nRT), we can set up the following proportion:
(2 liters N2) / (1 mole N2) = (V liters NH3) / (2 moles NH3)
From this proportion, we can deduce that:
V liters NH3 = (2 liters N2) * (2 moles NH3) / (1 mole N2)
Now, we need to determine the number of moles of N2 present in 2 liters. The molar volume of an ideal gas at standard temperature and pressure (STP) is approximately 22.4 liters. Therefore, the number of moles of N2 in 2 liters can be calculated as:
2 liters N2 / 22.4 liters/mole = 0.0893 moles N2
Substituting this value into the previous equation, we can find the volume of NH3:
V liters NH3 = (2 liters N2) * (2 moles NH3) / (0.0893 moles N2) ≈ 44.7 liters NH3
Therefore, when 2 liters of N2 is mixed with H2 at constant temperature and pressure, the volume of NH3 produced is approximately 44.7 liters.