CHEMISTRY COMMUNITY

"State whether reactants or products will be favored by an increase in the total pressure (resulting from compression) on each of the following equilibria. If there is no change, explain why that is so."

"(d) 2HD (g) + H2 -> D2 (g)"

Is this question a typo? The answer says no change because there are "the same number of moles of gas on both sides"

There isn't a typo; there are 2 moles of gas on the reactants' side (2 moles of HD) and 2 on the products' side (1 mole of H2 and 1 mole of D2). Thus, compression won't affect equilibrium.

The answer would be no change. This is due to the fact that there are an equal number of moles of gas on both sides of the reaction equation. Thus, an increase in pressure will not affect the equilibrium.

it is because you've copied down the problem incorrectly; the H2 is a product not a reactant :)

The reaction should be 2HD(g) --> H2(g) + D2(g). Therefore, there is an equal number of moles on each side.

Skyllar Kuppinger 1F wrote:it is because you've copied down the problem incorrectly; the H2 is a product not a reactant :)

There is a typo in the book.