ipl-logo

Molar Mass Of Benzoic Acid Lab Report

448 Words2 Pages

As mentioned earlier, the molar mass of benzaldehyde is 106.121g/mol, and the molar mass of benzoic acid is 122.12g/mol. With that in mind, to calculate the maximum possible mass of benzoic acid, which is the product of the experiment, Equation #2 must be used. Referencing from Table 1.1, the observed benzaldehyde mass is 5.02g, thus the plugging that into Equation #2, the calculation would be, (122.12 g⁄mol C_7 H_6 O_2)/(106.121 g⁄mol C_7 H_6 O)×5.02g, equaling to, 5.78g±0.01g of benzoic acid. To calculate the percentage yield, Equation #1, would be used, and the observed mass of benzoic acid, as stated in Table 1.1, is 5.68g, with the maximum benzoic acid possible to be 5.78g, as calculated using Equation #2. Thus, Equation #1 with the key information would look the following, 5.68g/5.78g×100%, equaling to a 98.3% yield, as shown in Table 2.1. …show more content…

Both the mass of benzoic acid and the mass of benzaldehyde have a mass error of ±0.01g, therefore, to calculate the percent error is by, ((0.01g/5.68g)+(0.01g/5.78g))×100%, equaling 0.3% error for the result. Converting the percent of percent yield to percent yield, the formula is the calculated percent error of the result divided by 100%, multiplied by the percentage yield. Therefore, 98.3%×((0.3%)/(100%)), equals to 0.2%, as demonstrated in Table 2.1, thus the final answer for the percent yield of benzoic acid is 98.2%±0.2%

Show More
Related
631 Words | 3 Pages

In this lab there were five different stations. For the first station we had to determine an unknown mass and the percent difference. To find the unknown mass we set up the equation Fleft*dleft = Fright*dright. We then substituted in the values (26.05 N * 41cm = 34cm * x N) and solved for Fright to get (320.5g). To determine the percent difference we used the formula Abs[((Value 1 - Value 2) / average of 1 & 2) * 100], substituted the values (Abs[((320.5 - 315.8) /

Read More
881 Words | 4 Pages

The percent recovery of the acid was 42%, but there was originally 40% of o-toluic acid in the mixture. The extra 2% could have been the impurity, 1, 4-dibromobenzene, which was isolated in the next part of the experiment. There is also another possible reason on why more acid was recovered. The acid wasn’t dried completely before it was weighed; the clumpy solids of the acid prove that it was still wet and thus, the extra liquid added to its mass. This could have been prevented by allowing the acid to dry longer or by drying it in an oven.

Read More
662 Words | 3 Pages

This low percent recovery is because some of the solutions spilled onto the table, losing a lot of the precipitate. The recovered ethyl-4-aminobenzoate’s boiling point was within the accepted range of 85C; meaning, the amount recovered was pure. The % recovery for the benzoic acid was 5.33%. This low percent recovery could be due to the fact that instead of adding NaCl to increase the precipitate amount, the salting out effect, more of the HCl was used. This caused the precipitate amount to increase slightly but not as much as it could’ve if the salting out effect was used.

Read More
230 Words | 1 Pages

The % yield was greater than 100% because the actual yield was greater than the theoretical yield. One error that may have caused this result to occur was that the copper may have not completely dried over the time it was left. If water was still inside the copper, it would increase the mass of the actual yield. If the copper was left in the beaker to dry for a longer time, it would help decrease the mass of the copper (as the water would be completely dried out) and bring the actual yield down.

Read More
256 Words | 2 Pages

1. What was your theoretical yield and your percent yield? Theoretical yield: 3.9151 g Percent yield: 79.30% 2. An accurate percent yield must be below 100% Why?

Read More
617 Words | 3 Pages

Name: Ashrith Epuri Lab Members: Ian, Averi, Serena Percent Yield Lab Objective: Determine the percent yield of NaCl in a chemical reaction. Materials: Evaporating dish Watch glass Digital balance Sodium bicarbonate Wire mesh Scoopula Plastic pipette Hydrochloric acid Hot plate Crucible tongs

Read More
1089 Words | 5 Pages

The solute in beaker 3 was isolated using gravity filtration and the rotovap and massed 0.283g. Due to the fact that there was originally 0.999g of the unknown mixture, it is assumed that half of the mass should have been in each beaker. However, that was not the case and the following percent recoveries were calculated: the percent recovery for 4-methylbenzoic acid was 55.8% and the percent recovery for 1,2-diphenylethane-1,2- dione was 56.6%. The calculated values for the percent recovery show that not all of the original mixture was recovered; reasons, as to why this may have occurred will be discussed

Read More
1442 Words | 6 Pages

The expected results were found through the theoretical mass calculations, equalling 52.39%. The experimental mass was 30.%, meaning that the percent error was 42%. These are the results due to the law of consevation of mass, and law of definite proportions, as discussed previously. The law of conservation of mass was used in this experiment because the assumption was made that mass could not be lost in the reaction. The differing masses between the start and end of the reaction was due to the release of carbon dioxide, meaning that mass was not destroyed, but located beyond the confines the utilized beaker.

Read More
807 Words | 4 Pages

The needed mass for reactant A was 3.52 grams and the needed mass for reactant B was 2.12 grams. The moles of product C (CaCO3) were also required to have been calculated using mass- to- mole conversion, but the mass was already established, so its mass was not calculated. Results Calculations used to determine the percent error 2.3 g CaCO3 - 2.00 g CaCO3 2.00 g CaCO3 x 100 = 15 % Reactants A and B’s masses were not similar, but the numbers were also not drastically different. Obviously, product C’s solution is different because moles were calculated as opposed to a mass.

Read More
728 Words | 3 Pages

For the first, the moles could be calculated by dividing the grams used by the molar mass of benzoic acid, 122.123. (NIH, 2016). .3/122.123= .0025 mol, which would then be divided by the volume of the solution, .065L. .0025/.0065=.378 M.

Read More
1184 Words | 5 Pages

The exact amount that is actually calculated during the end of the experiment is the actual yield, to calculate the percentage yield you must take the the actual yield

Read More
1146 Words | 5 Pages

The percent error compared to an ideal gas at STP (22.4 L) would then be: (22.43-22.4)/22.4×100=0.13%. These values compare well, meaning that little experimental error occurred during this part of the experiment. The universal gas constant for trial 3, turned out to be: 0.08199 (atm*L)/(mol*K). Compared with the ideal gas constant: 0.08206 (atm*L)/(K*mol), the percent error turned out to be 0.09% (above under “Trial 3 Calculations”). Thus, the value that was calculated from the experimental data was very close to the ideal constant, meaning again, little experimental error occurred during this part of the

Read More
1422 Words | 6 Pages

x 100% = percent composition (0.0326 mL / 1.00 mL) x 100% = 3.26% Average Percent Composition of H2O2 (3.26 % + 3.20 % + 3.36 %) / 3 = 3.27 % Trial Percent Composition of H2O2 1 3.26 % 2 3.20 % 3 3.36 % Average 3.27 % Balanced Redox Reaction: 2 MnO4- + 6 H+ + 5 H2O2 → 2 Mn2++ 8 H2O + 5

Read More
1054 Words | 5 Pages

℃^(-1)×6.40℃±3.1 %=1337.6 J±4.06 % ∆H=(-1337.6 J±4.06 %) /(0.025 mol ±0.16 %)= -53504 J m〖ol〗^(-1)±4.22 % ∆H=-53504 J m〖ol〗^(-1)±4.22 %÷1000=-54 kJ m〖ol〗^(-1)±4.22 % Conclusion and

Read More
1244 Words | 5 Pages

The percentage error with comparison to this value is 40.8%. This high percentage of error could be attributed to the various limitations and errors that were present in the experiment. Even though the bell peppers used were bought from the supermarket as a batch, this does not guarantee that the bell peppers were harvested at the same time. Thus, the inability to obtain fresh bell peppers could have resulted in this high percentage of error.

Read More

More about Molar Mass Of Benzoic Acid Lab Report

Open Document