Chemistry, 25.02.2020 19:53 chloegrace359

Aspirin can be made in the laboratory by reacting acetic anhydride (C 4H 6O 3) with salicylic acid (C 7H 6O 3) to form aspirin (C 9H 8O 4) and acetic acid (C 2H 4O 2). The balanced equation is
C 4H 6O 3+C 7H 6O 3?C 9H 8O 4+C 2H 4O 2
In a laboratory synthesis, a student begins with 2.80mL of acetic anhydride (density=1.08g/ml) and 1.24g of salicylic acid. Once the reaction is complete, the student collects 1.24g of aspirin.
Determine the limiting reactant for the reaction.
Determine the theoretical yield of aspirin for the reaction.
Determine the percent yield of aspirin for the reaction.

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Answer from: devo7420

The percent yield of the aspirin is 77.5 %.

Explanation:

To calculate the mass of acetic anhydride, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Density of acetic anhydride = 1.08 g/mL

Volume of acetic anhydride = 2.80 mL

Putting values in above equation, we get:

$1.08g/mL=\frac{\text{Mass of acetic anhydride}}{2.80mL}\\\\\text{Mass of acetic anhydride}=(1.08g/mL\times 2.80mL)=3.024g$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For acetic anhydride:

Given mass of acetic anhydride = 3.024 g

Molar mass of acetic anhydride = 102.1 g/mol

Putting values in equation 1, we get:

$\text{Moles of acetic anhydride}=\frac{3.024g}{102.1g/mol}=0.0296mol$

For salicylic acid:

Given mass of salicylic acid = 1.24 g

Molar mass of salicylic acid = 138.12 g/mol

Putting values in equation 1, we get:

$\text{Moles of salicylic acid}=\frac{1.24g}{138.12g/mol}=0.0089mol$

The chemical equation for the combustion of hexane follows:

$C_4H_6O_3+C_7H_6O_3\rightarrow C_9H_8O_4+C_2H_4O_2$

By Stoichiometry of the reaction:

1 mole of salicylic acid reacts with 1 mole of acetic anhydride

So, 0.0089 moles of salicylic acid will react with = $\frac{1}{1}\times 0.0089=0.0089mol$ of acetic anhydride

As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.

Thus, salicylic acid is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin

So, 0.0089 moles of salicylic acid will produce = $\frac{1}{1}\times 0.0089=0.0089moles$ of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.0089 moles

Putting values in equation 1, we get:

$0.0089mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=(0.0089mol\times 180.16g/mol)=1.60g$

To calculate the percentage yield of aspirin, we use the equation:

$\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Experimental yield of aspirin = 1.24 g

Theoretical yield of aspirin = 1.60 g

Putting values in above equation, we get:

$\%\text{ yield of aspirin}=\frac{1.24g}{1.60g}\times 100\\\\\% \text{yield of aspirin}=77.5\%$

Hence, the percent yield of the aspirin is 77.5 %.

Answer from: Quest

its first and third is your answer i did the qustion the fourth isnt right

Answer from: Quest

remember that hf is only the energy of one photon. not two. not three. one. 1) 5.12 * 10^3 photons find the energy of one photon, then determine how many photons are needed to reach the sensitivity. e = hf = (6.626 * 10^-34 js)(5.95 * 10^19 hz) = 3.94247 * 10^-14 j per photon (2.02 * 10^-10 j) / (3.94247 * 10^-14 j/photon) = 5123.69149 photons round to three sig figs. 2) 5.77 * 10^-17 j energy of pulse = energy per photon * number of photons = hfn = (6.626 * 10^-34 js)(1.66 * 10^13 hz)(5250) = 5.774559 * 10^-17 j round to three sig figs. 3) 4.07 * 10^8 kj/mol 10^12 pm = 1 m c = fλ f = c/λ e = hf = hc/λ = [(6.626 * 10^-34 js)(3.00 * 10^8 m/s) / (2.94 * 10^-12 m)](1 kj/1000 j)(6.02 * 10^23 photons/mol) = 40702571.4 kj/mol round to three sig figs. 4) 9.94 * 10^-1 m e = hc/λ λ = hc / e = (6.626 * 10^-34 js)(3.00 * 10^8 m/s) / (2.00 * 10^-25 j) = 0.9939 m round to three sig figs. 5) 9.06 * 10^3 photons energy of pulse = energy per photon * number of photons number of photons = energy of pulse / energy per photon = energy of pulse / (hf) = (3.87 * 10^-13 j) / [(6.626 * 10^-34 js)(6.45 * 10^16 hz)] = 9055.23695 photons round to three sig figs. 6) 2.78 * 10^-15 j this is problem 1, except in reverse. sensitivity = minumum number of photons * energy per photon = (5930)(6.626 * 10^-34 js)(7.077 * 10^14 hz) = 2.78070758 × 10^-15 j round to three sig figs.

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Aspirin can be made in the laboratory by reacting acetic anhydride (C 4H 6O 3) with salicylic acid (...

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