What is the consequences of increasing pressure on the equilibrium reaction ZnO(s) + H2(g) Zn(s) + H2O(I)?
According to Le Chatelier's Principle, increasing the pressure on a system at equilibrium will cause the equilibrium to shift toward the side with the fewer number of moles of gas to counteract the change.
ZnO(s) + H\(_2\)(g) → Zn(s) + H\(_2\)O(I)
Reactant side: Contains 1 mole of gas (H\(_2\)). Solid ZnO does not contribute to gas pressure.
Product side: Contains 0 moles of gas. Both Zn is a solid and H\(_2\)O is a liquid in this specific equation.
Result: Since the product side has fewer moles of gas (0 vs 1), increasing the pressure drives the equilibrium to the right (forward direction).
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