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University of Toronto

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Problem 87

Two successive reactions, D $\longrightarrow \mathrm{E}$ and $\mathrm{E} \longrightarrow \mathrm{F}$ , have yields of 48$\%$ and $73 \%,$ respectively. What is the overall percent yield for conversion of $\mathrm{D}$ to $\mathrm{F} ?$

Answer

$\eta=0,35$

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## Discussion

## Video Transcript

So we're giving the chemical reaction from D to ye and then you to half and from D to G and you two, you have to have a corresponding percentage you for 8% every 3%. So what will be the over or the scent issue from Detroit? Half. Um, the overall way essentially is multiplying individual percentage asked what percentage you office that So the overall weight. Oh, sorry Over said that you were because the 40% time Cimabue 3% and then it should be equals thio um off roughly around 35% and you can concentrate civil point for eight times 0.73 and then just notify the whole thing by 100% and then you will Finally, it's very 5%.

## Recommended Questions

Two successive reactions, $\mathrm{A} \longrightarrow \mathrm{B}$ and $\mathrm{B} \longrightarrow \mathrm{C},$ have yields of 73$\%$ and 68$\%$ , respectively. What is the overall percent yield for conversion of $\mathrm{A}$ to $\mathrm{C} ?$

One reaction in the production of sulfuric acid involves the conversion of sulfur dioxide to sulfur trioxide. In the presence of excess $\mathrm{O}_{2}, 88 \mathrm{kg} \mathrm{SO}_{2}$ produces $106 \mathrm{kg} \mathrm{SO}_{3}$ What is the percent yield?

The reaction of $15.0 \mathrm{g} \mathrm{C}_{4} \mathrm{HgOH}, 22.4 \mathrm{g} \mathrm{NaBr},$ and $32.7 \mathrm{g}$

$\mathrm{H}_{2} \mathrm{SO}_{4}$ yields $17.1 \mathrm{g} \mathrm{C}_{4} \mathrm{H}_{9} \mathrm{Br}$ in the reaction shown.

What are the (a) theoretical yield, (b) actual yield, and

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$\mathrm{C}_{4} \mathrm{H}_{9} \mathrm{Br}+\mathrm{NaHSO}_{4}+\mathrm{H}_{2} \mathrm{O}$.

In the reaction of $2.00 \mathrm{mol} \mathrm{CCl}_{4}$ with an excess of $\mathrm{HF}$,

$1.70 \mathrm{mol} \mathrm{CCl}_{2} \mathrm{F}_{2}$ is obtained.

$$\mathrm{CCl}_{4}+2 \mathrm{HF} \longrightarrow \mathrm{CCl}_{2} \mathrm{F}_{2}+2 \mathrm{HCl}$$

(a) The theoretical yield is $1.70 \mathrm{mol} \mathrm{CCl}_{2} \mathrm{F}_{2}$

(b) The theoretical yield is $1.00 \mathrm{mol} \mathrm{CCl}_{2} \mathrm{F}_{2}$

(c) The theoretical yield depends on how large an excess of HF is used.

(d) The percent yield is $85 \%$.

In the reaction of $277 \mathrm{g} \mathrm{CCl}_{4}$ with an excess of $\mathrm{HF}$, $187 \mathrm{g} \mathrm{CCl}_{2} \mathrm{F}_{2}$ is obtained. What are the (a) theoretical,

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$$\mathrm{CCl}_{4}+2 \mathrm{HF} \longrightarrow \mathrm{CCl}_{2} \mathrm{F}_{2}+2 \mathrm{HCl}$$.

What is the actual yield of a reaction? What is the percent yield of a reaction? How do the actual yield and the percent yield differ from the theoretical yield?

What is the percentage yield of a reaction?

For the reaction

$$\mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{O}_{2}(g)$$

the frequency factor $A$ is $8.7 \times 10^{12} \mathrm{s}^{-1}$ and the activation energy is $63 \mathrm{kJ} / \mathrm{mol} .$ What is the rate constant for the reaction at $75^{\circ} \mathrm{C} ?$

The activation energy $\left(E_{\mathrm{a}}\right)$ for the reaction

$2 \mathrm{N}_{2} \mathrm{O}(g) \longrightarrow 2 \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \Delta H^{\circ}=-164 \mathrm{kJ} / \mathrm{mol}$

is $240 \mathrm{kJ} / \mathrm{mol} .$ What is $E_{\mathrm{a}}$ for the reverse reaction?

a. What is the major monobromination product of the following reaction? Disregard stereoisomers.

b. What is the anticipated percent yield of the major product (as a percentage of all the monobrominated products)?