1- what is the \"experimental\" molecular weight of Benzoic Acid in g/mol the ma

Question

1- what is the "experimental" molecular weight of Benzoic Acid in g/mol the mass of benzoic acid is 1.068 g

the mass solvent is lauric acid= 8.084g

molality= 1.01

Tf= 38.3

kf=3.9

moles of benzoic acid = 0.01 mol

2- determine the accepted molecular weight for benzoic acid from its formula.

3- calculate the percent error.

4- what is the major sources of error in the experiment.

5- suppose your thermometers consistently read a temperature 1.2 lower than the correct temperature. how would this have affected the molar mass you found?

please I need answers for all 5 questions

thank you for help

Explanation / Answer

1. Given mass of benzoic acid = 1.068grams

Given moles of benzoic acid = 0.01moles

So, we know that moles = mass/molar mass

molar mass = mass/ moles = 1.068/0.01 = 106.81g/mol

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