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Amiraneli [1.4K]
3 years ago
13

What happens to acetone molecules when you add heat to a beaker of liquid acetone? They gain a higher average kinetic energy. Th

ey rearrange into a more ordered state. They get closer together. They move more slowly.
Chemistry
1 answer:
iVinArrow [24]3 years ago
7 0
When you heat up most substances it gives them more Kinetic energy and the substance becomes less arranged in an ordered state, further apart and move faster. therefore the answer is the first: They gain a higher average kinetic energy

Hope that helps :)
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The first part of a balanced chemical equation for a chemical reaction is shown below:
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According to the experimental procedure of Experiment F1, 135 microliters of acetophenone (120.15 g/mol, 1.03 g/mL) was reacted
Delicious77 [7]

Answer: The theoretical yield of 4-nitrochalcone is, 2.13\times 10^2

Explanation : Given,

Volume of acetophenone = 135  microliters = 135 × 10⁻⁶ L = 0.135 mL

conversion used : (1 microliter = 10⁻⁶ L) and (1 L = 1000 mL)

Density of acetophenone = 1.03 g/mL

Mass of acetophenone = Density × Volume = 1.03 g/mL × 0.135 mL = 0.139 g

Mass of 4-nitrobenzaldehyde = 127 mg  = 0.127 g

Conversion used : (1 mg = 0.001 g)

First we have to calculate the moles of acetophenone and 4-nitrobenzaldehyde

\text{Moles of acetophenone}=\frac{\text{Given mass acetophenone}}{\text{Molar mass acetophenone}}

\text{Moles of acetophenone}=\frac{0.139g}{120.15g/mol}=0.00116mol

and,

\text{Moles of 4-nitrobenzaldehyde}=\frac{\text{Given mass 4-nitrobenzaldehyde}}{\text{Molar mass 4-nitrobenzaldehyde}}

\text{Moles of 4-nitrobenzaldehyde}=\frac{0.127g}{151.12g/mol}=0.000840mol

Now we have to calculate the limiting and excess reagent.

The balanced chemical equation is:

C_8H_8O+C_7H_5NO_3\rightarrow C_{15}H_{11}NO_3

From the balanced reaction we conclude that

As, 1 mole of 4-nitrobenzaldehyde react with 1 mole of acetophenone

So, 0.000840 mole of 4-nitrobenzaldehyde react with 0.000840 mole of acetophenone

From this we conclude that, acetophenone is an excess reagent because the given moles are greater than the required moles and 4-nitrobenzaldehyde is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of 4-nitrochalcone

From the reaction, we conclude that

As, 1 mole of 4-nitrobenzaldehyde react to give 1 mole of 4-nitrochalcone

So, 0.000840 mole of 4-nitrobenzaldehyde react to give 0.000840 mole of 4-nitrochalcone

Now we have to calculate the mass of 4-nitrochalcone

\text{ Mass of 4-nitrochalcone}=\text{ Moles of 4-nitrochalcone}\times \text{ Molar mass of 4-nitrochalcone}

Molar mass of 4-nitrochalcone = 253.25 g/mole

\text{ Mass of 4-nitrochalcone}=(0.000840moles)\times (253.25g/mole)=0.21273g=212.73mg=2.13\times 10^2mg

(1 g = 1000 g)

Therefore, the theoretical yield of 4-nitrochalcone is, 2.13\times 10^2mg

4 0
3 years ago
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