## 5J.5 D

KeiannaPineda1B
Posts: 51
Joined: Mon Jun 17, 2019 7:24 am

### 5J.5 D

"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"

nicolely2F
Posts: 149
Joined: Sat Sep 14, 2019 12:17 am

### Re: 5J.5 D

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.

anjali41
Posts: 109
Joined: Fri Aug 09, 2019 12:15 am

### Re: 5J.5 D

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.

Skyllar Kuppinger 1F
Posts: 52
Joined: Thu Jul 25, 2019 12:16 am

### Re: 5J.5 D

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

kim 2I
Posts: 105
Joined: Thu Jul 25, 2019 12:17 am

### Re: 5J.5 D

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

KeiannaPineda1B
Posts: 51
Joined: Mon Jun 17, 2019 7:24 am

### Re: 5J.5 D

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.