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Hi! I don't think you would need to use PV= nRT. You would look at the Table and find that your Kc is 160 and then input the concentrations of [HI] and [I2] in the equilibrium constant equation to solve for x which is [H2].
Hello, as those above said, since they provide K and the equilibrium concentrations for HI and I2, you can solve H2 by setting up the equilibrium constant ratio, substituting in the values give, and solving for H2 that way. Hope this helps!
Ayesha Aslam-Mir 3C wrote:Would you use pv=nRT to solve this? You're not given a volume, so would we assume 1 L?
As others have mentioned above, this question asks you to refer to Table 5G.2 in order to get the Kc value! You can then use this value and set it equal to the K equation and solve for [H2].
I hope this was helpful!
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