Explore BrainMass
Share

Finding Kc from Products' Moles, Volume and Percent Reacted

This content was STOLEN from BrainMass.com - View the original, and get the already-completed solution here!

The following reaction occurs at 1600 deg. C.

Br2(g) <---> 2Br(g)

When 1.05 moles of Br2 are put in a 0.980 L flask, 1.20 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Kc for the reaction.

© BrainMass Inc. brainmass.com October 16, 2018, 10:35 am ad1c9bdddf - https://brainmass.com/chemistry/physical-chemistry/38920

Solution Summary

The solution provides an attachment containing the easy-to-follow calculations required to find the equilibrium constant Kc from the given data.

$2.19