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3 years ago

Calculations

Chemistry

2 answers:

Black_prince [1.1K]3 years ago

8 0

Answer:

Theoretical yield: 2.75g of paranitroaniline

Percentage yield: 54.5%

Explanation:

In strong-acid medium, acetanilide (Molar mass: 135.16g/mol) reacts producing para-nitroaniline (138.12g/mol) in a 1/1 reaction.

Theoretical yield of para-nitroaniline is the mass produced assuming a yield of 100%. That is:

2.7g acetanilide × (1mol / 135.16g) = 0.020 moles of acetanilide.

Assuming a yield of 100% are 0.020 moles of paranitroaniline. Theoretical yield is:

0.020 moles × (138.12g / mol) =

<h3>Theoretical yield: 2.75g of paranitroaniline</h3><h3 />

Percentage yield is:

(Actual yield / theoretical yield) × 100

Actual yield was 1.5g and percentage yield will be:

Percentage yield: (1.5g / 2.75g) × 100

<h3>Percentage yield: 54.5%</h3>

Mashutka [201]3 years ago

7 0

Don’t mind me just trying to get some points

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Strong acids are which ionize completely in aqueous solution into hydrogen ions and the corresponding anion. Examples of strong acids include hydrobromic acid, hydrochloric acid, tetraoxosulfate (vi) acid.

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Part B:

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Answer:

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Explanation:

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We have given in the question

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And $R$ is the Universal Gas Constant.

$R=0.008 314 kJ/Kmol$

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Taking inverse log both side we get,

$\frac{P_2}{102}=e^{1.165}\\\\P_2=102\times 3.20\ mmHg\\P_2=327\ mmHg$

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