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Elodia [21]
3 years ago
5

Classify each of the following compounds as an acid, base, or both. Be sure to answer all parts.

Chemistry
1 answer:
Oduvanchick [21]3 years ago
6 0

Explanation:

According to Bronsted-Lowry an acid is defined as the specie which is able to donate hydrogen ions when dissolved in water.

For example, HCl \rightarrow H^{+} + Cl^{-}

On the other hand, bases are the species which are able to donate hydroxide ions when dissolved in water.

For example, NaOH \rightarrow Na^{+} + OH^{-}

In CH_{3}CH_{2}OH compound, when it will lose hydrogen ion then it will result in the formation of a CH_{3}CH_{2}O^{-} (alkoxide ion). As the carbon atoms are donating their positive charge towards the O^{-} ion so, it will become unstable in nature.

As a result, it will neither give a hydrogen ion or a hydroxide ion.

In CH_{3}CH_{2}CH_{2}CH_{3}, there is no difference in the electronegativity of both carbon and hydrogen atoms. Therefore, this compound is not polar in nature hence, it will neither give a hydrogen or hydroxide ion.

In CH_{3}CO_{2}CH_{3} there is presence of no -OH group. Hence, it will neither give a hydroxide or hydrogen ion.

Thus, we can conclude that none of the given compounds will act as an acid or a base.

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tatuchka [14]

Answer:

See explanation and images attached

Explanation:

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b)  In the second mechanism, an unnamed ester is hydrolysed using an acid catalyst. The attack of the acid and subsequent nucleophillic attack of water labelled with 18O leads to the incorporation of this 18O into the product acid as shown in the mechanism attached to this answer.

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FrozenT [24]
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Create the Equation: What is the Percent Yield of Ammonia (NH3) if 11.8 g is recovered in a reaction with 7.02 x 10^23 molecules
insens350 [35]

Answer:

Explanation:

The first thing that you need to do here is to calculate the theoretical yield of the reaction, i.e. what you get if the reaction has a

100

%

yield.

The balanced chemical equation

N

2

(

g

)

+

3

H

2

(

g

)

→

2

NH

3

(

g

)

tells you that every

1

mole of nitrogen gas that takes part in the reaction will consume

3

moles of hydrogen gas and produce

1

mole of ammonia.

In your case, you know that

1

mole of nitrogen gas reacts with

1

mole of hydrogen gas. Since you don't have enough hydrogen gas to ensure that all the moles of nitrogen gas can react

what you need

3 moles H (sub 2)

>

what you have

1 mole H (sub2)

you can say that hydrogen gas will act as a limiting reagent, i.e. it will be completely consumed before all the moles of nitrogen gas will get the chance to take part in the reaction.

So, the reaction will consume

1

mole of hydrogen gas and produce

1

mole H

2

⋅

2 moles NH

3

3

moles H

2

=

0.667 moles NH

3

at

100

%

yield. This represents the reaction's theoretical yield.

Now, you know that the reaction produced

0.50

moles of ammonia. This represents the reaction's actual yield.

In order to find the percent yield, you need to figure out how many moles of ammonia are actually produced for every

100

moles of ammonia that could theoretically be produced.

You know that

0.667

moles will produce

0.50

moles, so you can say that

100

moles NH

3

.

in theory

⋅

0.50 moles NH

3

.

actual

0.667

moles NH

3

.

in theory

=

75 moles NH

3

.

actual

Therefore, you can say that the reaction has a percent yield equal to

% yield = 75%

−−−−−−−−−−−−−

or 75 moles NH sub3

I'll leave the answer rounded to two sig figs.

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dlinn [17]
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