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Volgvan
3 years ago
11

The Wolff–Kishner reaction uses hydrazine (H2NNH2) and hydroxide (–OH) to reduce a carbonyl to the alkane. The first steps of th

e mechanism convert a carbonyl to a hydrazone in a manner similar to imine formation. Draw the mechanism arrows for the reaction from the hydrazone to the alkane. Be sure to add lone pairs of electrons and nonzero formal charges to all species.
Chemistry
1 answer:
valentina_108 [34]3 years ago
8 0

Your answer would be D.

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Consider the reaction:
Fofino [41]

The mass in grams of NH₃ produced from the reaction is 3.4 g

<h3>Balanced equation</h3>

We'll begin by writing the balanced equation for the reaction. This illustrated below:

N₂ + 3H₂ -> 2NH₃

From the balanced equation above,

1 dm³ of N₂ reacted to produced 2 dm³ NH₃

<h3>How to determine the volume of NH₃ produced</h3>

From the balanced equation above,

1 dm³ of N₂ reacted to produced 2 dm³ NH₃

Therefore,

2.24 dm³ of N₂ will react to produce = 2.24 × 2 = 4.48 dm³ of NH₃

<h3>How to determine the mass of NH₃ produced</h3>

We'll begin by obtained the mole of 4.48 dm³ of NH₃. Details below:

22.4 dm³ = 1 mole NH₃

Therefore,

4.48 dm³ = 4.48 / 22.4

4.48 dm³ = 0.2 mole of NH₃

Finally, we shall determine the mass of NH₃ as follow:

  • Molar mass of NH₃ = 17 g/mol
  • Mole of NH₃ = 0.2 mole
  • Mass of NH₃ =?

Mass = mole × molar mass

Mass of NH₃ = 0.2 × 17

Mass of NH₃ = 3.4 g

Learn more about stoichiometry:

brainly.com/question/13196642

#SPJ1

4 0
2 years ago
Which of the following representations shows the correct placement of trophic levels?
OleMash [197]
You have to start listing from the bottom :

3. Secondary Consumers

2. Primary Consumers

1. Producer

4 0
3 years ago
How do you figure out how many isotopes an element has?
Helen [10]

by counting the isoto

7 0
3 years ago
2Al2O3 (s) + 3C (s) LaTeX: \longrightarrow ⟶ 4Al (s) + 3CO2 (g)
densk [106]

Answer:

Percent yield = 79.79 %

Explanation:

Given data:

Mass of Al₂O₃ = 821 g

Mass of Al = 349 g

Percent yield = ?

Solution:

Chemical equation:

2Al₂O₃ + 3C     →      4Al  + 3CO₂

Number of moles of Al₂O₃:

Number of moles = mass/molar mass

Number of moles = 821 g/ 101.96 g/mol

Number of moles = 8.1 mol

Now we will compare the moles of Al with Al₂O₃.

                Al₂O₃        :         Al

                    2           :          4

                  8.1           :      4/2×8.1 = 16.2 mol

Mass of Al:

Mass = number of moles × molar mass

Mass = 16.2 mol ×  27 g/mol

Mass = 437.4 g

Percent yield:

Percent yield = (actual yield / theoretical yield)× 100

Percent yield =  (349 g/ 437.4 g) × 100

Percent yield = 79.79 %

6 0
3 years ago
I did not mean to publish this ;-;
san4es73 [151]

Answer:

dang

Explanation:

6 0
3 years ago
Read 2 more answers
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