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aleksandr82 [10.1K]

1 year ago

12

What products do you expect from the reaction, after acidifying the reaction mixture?

1 answer:

soldi70 [24.7K]1 year ago

8 0

Cl3C --OH

Cl3C ---Oh products do you expect from the reaction, after acidifying the reaction mixture.

What is acidifying?

Lowering a sample's pH below 2.0 by adding an acid (often nitric or sulfuric). A sample is fixed by acidification in order to prevent change until it is analysed.

Therefore,

What products do you expect from the reaction, after acidifying the reaction mixture?

Cl3C --OH

Cl3C ---Oh Oh products do you expect from the reaction, after acidifying the reaction mixture.

To learn more about acidifying from the given link:

brainly.com/question/24255408

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What is “monomer” mean?

oksano4ka [1.4K]

it is a molecule* that can be joined with other molecules that are identical to form a polymer*

key words :

a molecule:

a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction.

a polymer:

a substance that has a molecular structure consisting chiefly or entirely of a large number of similar units bonded together

hope this helped, good luck in future studies !

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Ronch [10]

D will be the answer I hope that help good luck I hope. My answer help you

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When methane ( CH4 ) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reac

slega [8]

<h2>Answer:</h2> $1.33*10^{-2}grams$

<h2>Explanations</h2>

The complete balanced equation for the given reaction is expressed as;

$CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g)$

Given the following parameters

Mass of CH4 = 5.90×10^−3 g = 0.0059grams

Determine the moles of methane

$\begin{gathered} moles\text{ of CH}_4=\frac{mass}{molar\text{ mass}} \\ moles\text{ of CH}_4=\frac{0.0059}{16.04} \\ moles\text{ of CH}_4=0.000368moles \end{gathered}$

According to stoichimetry, 1 mole of methane produces 2 moles of water, hence the moles of water required will be:

$\begin{gathered} moles\text{ of H}_2O=\frac{2}{1}\times0.000368 \\ moles\text{ of H}_2O=0.000736moles \end{gathered}$

Determine the mass of water produced

$\begin{gathered} Mass\text{ of H}_2O=moles\times molar\text{ mass} \\ Mass\text{ of H}_2O=0.000736\times18.02 \\ Mass\text{ of H}_2O=0.0133grams=1.33\times10^{-2}grams \end{gathered}$

Therefore the mass of water produced from the complete combustion of 5.90×10−3 g of methane is 1.33 * 10^-2grams

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Mashutka [201]

Answer:

Potential

Explanation:

The answer is potential!

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