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### Q 11.47

Posted: **Fri Jan 11, 2019 7:51 am**

by **Riya Shah 4H**

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)?

### Re: Q 11.47

Posted: **Fri Jan 11, 2019 2:14 pm**

by **Katelyn Pham 4E**

First you'd have to make an ICE table.

### Re: Q 11.47

Posted: **Fri Jan 11, 2019 2:34 pm**

by **Emilia z**

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

### Re: Q 11.47

Posted: **Mon Jan 14, 2019 3:09 pm**

by **Laura Gong 3H**

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.