Predict how the total pressure varies during the gas-phasereaction N2 (g) + 3 H2(g) = 2 NH3 (g) in a constant-volumecontainer
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Predict how the total pressure varies during the gas-phase reaction N2(g)+3 H2(g) 2 NH3(g) in a constant-
At a fixed temperature, equal moles of N2 (g) and H2 (g) are mixed in a constant pressure container (the volume of the container changes in order to keep the pressure at a constant value). The N2 (g) and H2 (g) are allowed to react, producing NH3 (g):
N2 (g) + 3 H2 (g) ? 2 NH3 (g)
If the initial volume of the container, before any reaction takes place, is 4.60 L, determine the volume of the container after the N2 (g) and H2 (g) have reacted to completion.
Nitrogen and hydrogen gases react to form ammonia gas as follows:
N2(g) + 3 H2(g) 2 NH3(g)
At a certain temperature and pressure, 1.2 L of N2 reacts with 3.6 L of H2. If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?