Q 11.47

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Riya Shah 4H
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Joined: Wed May 02, 2018 3:00 am

Q 11.47

Postby Riya Shah 4H » Fri Jan 11, 2019 7:51 am

For the reaction PCl5(g) (equilibrium arrow) PCl3(g) + Cl2(g), Kc = 1.1 X 10^-2 at 400. K. (a) Given that 1.0 g of PCl5 is placed in a 250.-mL reaction vessel, determine the molar concentrations in the mixture at equilibrium. (b) What percentage of the PCl5 has decomposed at equilibrium at 400. K?

Could someone please tell me the quadratic equation for this and how to do (b)?

Katelyn Pham 4E
Posts: 30
Joined: Fri Sep 28, 2018 12:21 am

Re: Q 11.47

Postby Katelyn Pham 4E » Fri Jan 11, 2019 2:14 pm

First you'd have to make an ICE table.

Emilia z
Posts: 28
Joined: Fri Sep 28, 2018 12:21 am

Re: Q 11.47

Postby Emilia z » Fri Jan 11, 2019 2:34 pm

First you have to use an ICE table to find the concentrations at equalibrium (to get your quadratic you should use the equation for K and your given K value), then you can use those numbers to figure out the percent that decomposed for part b

Laura Gong 3H
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Re: Q 11.47

Postby Laura Gong 3H » Mon Jan 14, 2019 3:09 pm

To solve for the percentage of PCl5 decomposed, I found the percentage of PCl5 remaining and divided it by the initial amount of PCl5. Once I found that percentage, I subtracted that value from 1 to get the percentage of PCl5 decomposed.

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