Reactions of Ethers and Epoxides 18-44 Predict the products of the following ether cleavage reactions: (a) (b) CH3 CH2CH3 CF3CO2H H20 2 H3C CH3 HI 7 (c) CH3 H2C=CH-0-CH2CH3 HI H2O ? (d) CH3CCH2-O-CH2CH3 CH3 HI H20 ?

Answers

Answer 1

The product would be: a. [tex]CH_3CH_2^+ + CH_3CH_2OH + CF_3CO^{2-}[/tex]

b. [tex]H_3C-I + CH_3CH_2-I + H_2O[/tex]

c. [tex]H_3CCH_2OH + CH_3CH_2I[/tex]

d. [tex]CH_3CCH_2OH + CH_3CH_2I[/tex]

(a) The reaction of an ether with a strong acid like [tex]CF_3CO_2H[/tex] can lead to the cleavage of the ether bond and the formation of two carbocations. In this case, the product would be:

[tex]CH_3CH_2^+ + CH_3CH_2OH + CF_3CO^{2-}[/tex]

(b) The reaction of an ether with HI can lead to the cleavage of the ether bond and the formation of two alkyl halides. In this case, the product would be:

[tex]H_3C-I + CH_3CH_2-I + H_2O[/tex]

(c) The reaction of an ether with HI and subsequent reaction with water can lead to the formation of an alcohol and an alkyl halide. In this case, the product would be:

[tex]H_3CCH_2OH + CH_3CH_2I[/tex]

(d) The reaction of an ether with HI and subsequent reaction with water can lead to the formation of an alcohol and an alkyl halide. In this case, the product would be:

[tex]CH_3CCH_2OH + CH_3CH_2I[/tex]

Note that in both (c) and (d), the reaction can proceed via an SN1 mechanism in which the leaving group (the ether oxygen) departs to form a carbocation intermediate.

The carbocation can then react with the nucleophilic iodide ion to form the alkyl halide, while the protonated alcohol can undergo deprotonation to form the final alcohol product.

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CORRECT QUESTION

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Reactions Of Ethers And Epoxides 18-44 Predict The Products Of The Following Ether Cleavage Reactions:
Answer 2

(a) Acid-catalyzed hydrolysis reaction

(b) Nucleophilic substitution reaction

(c) Nucleophilic substitution reaction

(d) Acid-catalyzed hydrolysis reaction

When it comes to predicting the products of ether cleavage reactions, it's important to consider the specific conditions of each reaction. Here are the predictions for the reactions you provided:

(a) CH3 CH2CH3 CF3CO2H H20 2 H3C CH3
This is an acid-catalyzed hydrolysis reaction, which will break the ether bond and form two alcohol products. The specific products will depend on the specific ether being cleaved, but in general, the products will be a primary alcohol (CH3CH2OH) and a tertiary alcohol (H3CCH3OH).

(b) HI 7
This is a classic example of a nucleophilic substitution reaction, in which the iodide ion (I-) acts as a nucleophile and attacks the ether carbon to break the bond and form an alkyl iodide product. In this case, the products will be H3CCH2I and CH3I.

(c) CH3 H2C=CH-0-CH2CH3 HI H2O
This reaction is also a nucleophilic substitution reaction, but the specific conditions are different. In this case, the hydroxide ion (OH-) from water acts as a nucleophile to attack the ether carbon and break the bond. The products will be H3CCH=CH2 (an alkene) and CH3OH (a primary alcohol).

(d) CH3CCH2-O-CH2CH3 CH3 HI H20
This is another acid-catalyzed hydrolysis reaction, similar to part (a). The ether bond will be broken and two alcohol products will be formed. The specific products will depend on the specific ether being cleaved, but in general, the products will be a primary alcohol (CH3CH2OH) and a secondary alcohol (CH3CH2CH2OH).

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—Evidence—

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N2 + 3H2 → 2NH3 How many grams of hydrogen are necessary to react completely with 853.42g of nitrogen in the above reaction?

Answers

Answer: 182.87 grams of hydrogen are necessary to react completely with 853.42g of nitrogen.

Explanation:

The balanced chemical reaction is :

[tex]N_2+3H_2\rightarrow 2NH_3[/tex]

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]  

[tex]\text{Number of moles of nitrogen}=\frac{853.42g}{28g/mol}=30.479moles[/tex]

According to stoichiometry:

1 mole of [tex]N_2[/tex] react with = 3 moles of [tex]H_2[/tex]

30.479 moles of [tex]N_2[/tex] will react with=[tex]\frac{3}{1}\times 30.479=91.437moles[/tex] of [tex]H_2[/tex]

 Mass of [tex]H_2[/tex] =[tex]moles\times {\text {Molar mass}}=91.437mol\times 2g/mol=182.87g[/tex]

Thus 182.87 grams of hydrogen are necessary to react completely with 853.42g of nitrogen.

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Answer:

A lot of people rejected it outright. Christians were persecuted and killed for their beliefs, and there were no cars, etc for easy transportation. Most people had to walk everywhere since horses and the like were only for the rich and royal. Hope this helps, please give me brainliest :)

Explanation:

Answer: Your not the best a spelling...

Explanation:

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PLEASE HELP!!!

How many kilograms of chlorine gas is needed to produce 45.0 grams of hydrochloric acid?

Answers

Answer:

43.76 g = 0.04376 Kg

Explanation:

The equation of the reaction is given as;

H2 + Cl2 --> 2HCl

From the equation;

1 mol of Cl2 produces 2 mol of HCl

Converting to mass;

Mass = Number of mol * Molar mass

Cl2;

Mass = 1 mol * 70.906 g/mol = 70.906 g

HCl;

Mass = 2 mol * 36.458 g/mol = 72.916 g

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70.906 g of Cl2 produces 72.916 g of HCl

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A gas has a volume of 500cm3 when a pressure of 100,00N is exacted on it what will be it's volume if the pressure is changed to 150mm mecury at same temperature

Answers

Answer:

See explanation below

Explanation:

At first sight, it seems that the innitial pressure of 100,00 N would be 100,00 N/m² because pressure does not have units of newton alone. If this is true, then the calculations are the following (If it's not, but it's actually mm Hg, then skip the part of the conversion, and just do the procedure of solving for the volume).

The innitial pressure is 100 N/m² or simply 100 Pa. As the second pressure is in mm Hg, let's convert the Pascal units to mm Hg:

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X = 100 * 0.007501 / 1 = 0.7501 mmHg

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Using this expression, let's solve for V₂:

V₂ = 0.7501 *¨500 / 150

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Now, it's the innitial pressure is 100 mm Hg then the volume:

V₂ = 100 * 500 / 150

V₂ = 333.33 cm³

Check the units of the innitial pressure, one of these results should be the correct answer. If it's not, then please post again the question with the correct units.

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Answers

Answer:

A glass of mineral water is not pure water.

Explanation:

Pure chemical substances

Pouring water into a glass from a bottle

Food and drink may be advertised as ‘pure’. For example, you may see cartons of ‘pure orange juice’ or ‘pure mineral water’. This means that nothing else was added to the orange juice or mineral water during manufacture. However, these substances are not pure to a scientist. In science, a pure substance contains only one element or compound.

Mineral water is mostly water, but there are other substances mixed with it. These are the ingredients that you see listed on the bottle’s label.

Elements and compounds are usually more dense in their solid than in their
liquid state. However, water is one of the notable exceptions. The density
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Answers

Explanation:

The molecules in water is more tightly packed than in ice, so water has greater density than ice.

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