what would have happened to the calculated molar mass if some benzoic acid was spilled before adding it to the lauric acid?

also, what would have happened to the calculated molar mass if the thermometer used actually read 1.4C too high

I NEED HELP PLEASE

THANKS

Which was the solute and which the solvent? I'm assuming from the question I answered last night about lauric acid that the lauric acid is the solute and benzoic acid is the solvent.

(1)delta T = Kf*m
(2) m = mols/kg solvent
(3) mols = grams/molar mass

Follow from the equations above.
If the benzoic acid is the solvent and you spilled some of it then the m of the solution will be too large from equation 2; i.e., m = mols/kg solvent. If kg solvent is smaller the m is larger from equation 2 and that makes delta T larger from equation 1. Now we go forward.
larger dT in 1 gives larger m, larger m in 2 gives larger mols, larger mols in 3 gives smaller molar mass.

If the thermometer read too high by 1.4 or too low by 1.4 (actually too high or too low by essentially any number) the molar mass is not affected. Why? Because you read 1.4 degrees too high BOTH times so delta T remains the same. Here is an example. Let's say the reading on a good thermometer is 0C for water as the normal freezing point and -10 for the new freezing point so delta T is 0-(-10) = 10 C.
Now lets use the "bad" thermometer which reads too high by 2C (make it easier to calculate). So instead of reading 0 for the normal freezing point it will read +2. Then the NEW freezing point for the solution will be -10+2 = -8. Now delta T = +2-(-8) = 10. Voila!
As long as you measure DELTA T it makes little difference whether it is all that accurate BUT you want it to be "off" by the same amount for every reading you make..

thanks

If some benzoic acid was spilled before adding it to the lauric acid, the calculated molar mass of the resulting mixture would be lower than expected. This is because the spilled benzoic acid would not have contributed to the total mass of the mixture, resulting in a lower overall mass for the calculation of molar mass.

On the other hand, if the thermometer used actually read 1.4°C too high, the calculated molar mass of the substance being measured would be affected. This is because temperature is an important factor in determining the molar mass of a substance using the ideal gas law equation.

The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. In this equation, if the temperature is higher than the actual value, it would result in a larger value for the molar mass. Conversely, if the temperature is lower than the actual value, it would produce a smaller value for the molar mass. In this case, if the thermometer read 1.4°C too high, the calculated molar mass would be higher than the true value.

It's important to note that both scenarios would lead to discrepancies in the calculated molar mass, which could impact the accuracy of any subsequent calculations or analysis.

If some benzoic acid was spilled before adding it to the lauric acid, the calculated molar mass would be affected. In order to understand how, we need to know the steps involved in calculating the molar mass.

The molar mass of a compound is determined by summing up the atomic masses of all the elements present in it. Typically, in a laboratory setting, we measure the mass of a compound and the amount of substance (in moles) to calculate molar mass.

In this case, it seems like you are conducting an experiment involving a mixture of benzoic acid and lauric acid. Usually, a known mass of each compound is measured and added together to obtain the total mass, which is then used to calculate the molar mass. However, if some benzoic acid is spilled before adding it to the lauric acid, the actual mass of the benzoic acid used will be less than the intended mass. This means that the total mass used in the calculation will be lower than expected, leading to a lower calculated molar mass.

Now let's consider the situation with the thermometer. If the thermometer used actually reads 1.4°C too high, this will affect any temperature measurements taken during the experiment. Temperature is often used in calculations, such as determining the amount of substance based on temperature-dependent conversions.

For example, if you are using a temperature-dependent conversion equation or formula, a higher measurement of temperature will result in a different value for the calculated amount of substance. This, in turn, will affect the calculated molar mass.

To obtain accurate results in the experiment, it is essential to minimize any sources of error, such as spills or incorrect instrument readings. However, if these errors do occur, recognizing their impact on the calculations can help you make more accurate adjustments or interpretations.