11.73 6th edition

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Jeremiah Hutauruk
Posts: 67
Joined: Fri Sep 28, 2018 12:28 am

11.73 6th edition

Postby Jeremiah Hutauruk » Tue Jan 15, 2019 11:04 pm

11.73 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.
(a) 2 O3(g) ∆ 3 O2(g)
(b) H2O(g) C(s) ∆ H2(g) CO(g)
(c) 4 NH3(g) 5 O2(g) ∆ 4 NO(g) 6 H2O(g) (d) 2 HD(g) ∆ H2(g) D

Jane Burgan 1C
Posts: 73
Joined: Fri Sep 28, 2018 12:15 am

Re: 11.73 6th edition

Postby Jane Burgan 1C » Tue Jan 15, 2019 11:42 pm

I can't really tell what the equations are because it looks like the computer keyboard may have messed them up haha but I think for a it's reactants because there are more moles of gas on the right side of the reaction. In general for these problems, you can figure them out by this rule : if there are more moles of gas on the right side of the reaction then reactants will be favored but if there are more moles of gas on the left side of the reaction then products will be favored!

Sophia Ding 1B
Posts: 62
Joined: Fri Sep 28, 2018 12:16 am

Re: 11.73 6th edition

Postby Sophia Ding 1B » Wed Jan 16, 2019 4:22 pm

The rule that Jane said about which side will be favored (which ever has less will be favored) is a handy trick, but just remember also that if there is the use of an inert gas to increase pressure of the system, then the system will remain at equilibrium as the gas has no real affect on neither the reactants nor products.


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