I'm looking for the solution to problem 111 in Chapter 6 of Introduction to General, Organic and Biochemistry 11th Edition (Bettelheim, Capbell, Brown...). I do not have the textbook in front of me to supply the question. This problem has yet to be answered in the solution section upon review.

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!!!PLEASE READ MY QUESTION BEFORE DOING ANYTHING!!!

Let's try this again! What I'm looking for is an explanation. NOT A SOLUTION.

So I have the answer and it's correct(obviously right), but my question is why was K_p2 multiplied with itself. In other words, why did I have to (K_p2)² X K_p1 ?

Since K_p2 is a reverse reaction of K_p1 shouldn't K_p2 be (1/K_p2)² ?

What are the directions to calculate something like this

I have been working on this question. I do not know wheretostart. Could you please show me how to start and work throughthisquestion? I beleive its a delta change of freezing pointdepressionquestion, and im pretty sure that you have to figure outthemolarity of all the compounds in the molecular formula, yet imnotsure what effect burning has on the problem. Futhermore,Iunderstand its a multiple step problem and it is reallyconfusingme.

Here is the question:

A compound of carbon, hydrogen, and oxygen was burnedinoxygen, and 1.000g of the compound produced 1.418 g CO2 and .871gH2O. In another experiment, .1103 g of the compound wasdissolvedin 45.0 g of water. This solution had a freezing point of-0.0734degrees C. What is the molecular formula of thecompound?

I'm having trouble with doing the assignment in the box correctly. Can anyone help me out? thank you!

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I'm looking for the solution to problem 111 in Chapter 6 of Introduction to General, Organic and Biochemistry 11th Edition (Bettelheim, Capbell, Brown...). I do not have the textbook in front of me to supply the question. This problem has yet to be answered in the solution section upon review.

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