Step-by-step explanation:
We have this reaction: 2H2(g) + O2(g) -> 2H2O(g) + energy
It is an exothermic reaction, so the ΔH is negative
Temperature
Increasing the temperature of an equilibrium reaction favors the molecules to collide more, while decreasing the temperature reduces their agitation and, consequently, the shocks. An increase in temperature always favors an endothermic reaction (one that absorbs energy).
The analysis of the effect of temperature on an equilibrium mainly takes into account the ΔH of the reaction. If ΔH is positive, the forward reaction will be endothermic, while the reverse will be exothermic. If ΔH is negative, the forward will be exothermic and the inverse, endothermic.
In this case, we have an exothermic reaction, so if we increase the temperature, there is a reverse shift in the reaction.
If we decrease the temperature, there is a forward shift in the reaction.
Pressure
The pressure variation only promotes displacement in equilibria that present gaseous components, since when it is increased the molecules increase the shocks among themselves, and when the pressure is decreased, they decrease the shocks among themselves.
The collisions between molecules increase with increasing pressure, because the volume (space) is consequently decreased, while the decrease in pressure is accompanied by an increase in volume.
In chemical equilibrium, the analysis of the effect of pressure modification takes into account the molar volume of reactants and products, which volume is related to the reaction coefficients.
According to Le Chatelier's principle, if the pressure of a system is increased, the equilibrium will shift towards the smaller volume, while if the pressure is decreased, the equilibrium will shift towards the larger volume side.
So in this case, if we increase the pressure, there is a forward shift in the reaction.
Concentration of H2, O2 and H2O
When the concentration in amount of matter (in mol/L or molar) of a participant in the reaction is changed (either decreased or increased), the equilibrium shift will occur, provided that participant is not in the solid state.
Thus, according to Le Chatelier's principle, if the concentration of a participant is increased, the equilibrium will shift in the opposite direction to the increase. However, if the participant's concentration is reduced, the equilibrium will shift in the direction of decrease.
So in this case, if we increase the amount of H2, there is a forward shift in the reaction.
If we remove O2, there is a reverse shift in the reaction.
If we increase the amount of H2O, there is a reverse shift in the reaction.
Answer:
if we increase the temperature, there is a reverse shift in the reaction.
If we decrease the temperature, there is a forward shift in the reaction.
if we increase the pressure, there is a forward shift in the reaction.
if we increase the amount of H2, there is a forward shift in the reaction.
If we remove O2, there is a reverse shift in the reaction.
If we increase the amount of H2O, there is a reverse shift in the reaction.