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11 Dec 2019

Urea is hygroscopic, meaning it attracts water. If the lab is very humid and the bottle of urea is open for a long time, some water molecules will stick to urea. What do you expect is the change/are the changes of the melting point?

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Nelly Stracke
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13 Dec 2019
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Related questions

I went through these two problems the simplest way I could find,using the formula:

ΔH°f298 = ΣνiΔH°i

1. In order to determine the ΔH°f298 for urea, Peter decides tocarry out a calorimetric analysis. He determines that the heat ofcombustion of urea, (NH2)2CO(s), at 25°C is 589,000 J mol-1 whenthe products are CO2(g), H2O(l), and N2(g). Calculate ΔH°f298 forurea at this value?It is later found that the previous analysis hadsome errors and that the heat of combustion of urea is actually603,200 J mol-1. By how much does the ΔH°f298 change?

2. What are the standard heats of combustion of methane andpropane gas at 25°C if the combustion products are H2O(l) andCO2(g)?

For problem 1.) I got -963000J/mol for the heat of formationoriginally, and -991000J/mol.

2.) I got -891000J/mol for methane, and -2220000J/mol.

How far am I off and how do I fix this?


What is the purpose of performing mixed melting point experiments? For example, if your unknown is phenacetin, what do you expect to see with a mixed melting point experiment using your unknown and phenacetin out of a bottle? What do you expect to see with a mixed melting point using your unknown and acetanilide out of a bottle?

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