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# Iron (D1) hydroxide decomposes in the following reaction: 2 FE(OH)3 (S) &lt;_&gt; F6203 (S) + 3 H20(g). For this reaction, Kp=2.35 at 300C. If you

I'm having trouble figuring out how to solve this problem, I know we have to use an ice table to find unknown variables but Im not sure how to go about solving for all of the parts. Please explain your answer and show all the steps and rationale behind solving this problem. Its greatly appreciated! Thank you!!

Iron (D1) hydroxide decomposes in the following reaction:
2 FE(OH)3 (S) &lt;_—&gt; F6203 (S) + 3 H20(g). For this reaction, Kp=2.35 at 300°C. If you put 9.5 g of iron (D1) hydroxide in a 2.3 L
container and heat it to 300°C, what percentage of the iron (D1) hydroxide will decompose? A) 43.7%
B) 14.9%
C) 78.1%
D) 24.3%
E) 93.2%

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