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Debora [2.8K]
3 years ago
15

Which example best demonstrates Charles’s law?

Chemistry
2 answers:
Liono4ka [1.6K]3 years ago
6 0

Answer:

A

Explanation:

The Charles law states that the volume of an ideal gas increases when temperature is increased under constant pressure. The pressure inside the balloon is always equal to the atmospheric pressure. Therefore answer A demonstrate the Charles law.

Assoli18 [71]3 years ago
6 0

<u>Answer:</u>

<em>D.  A syringe pulls in air as the plunger is pulled back.</em>

<u>Explanation:</u>

As per Charles’s law  

At constant pressure for a given amount of a gas,

Volume is directly proportional to its temperature.

Directly proportional means when one increases the other one too will increase. That is when volume increases temperature too will increase. When volume decreases, temperature too will show a decrease.

Option A tells us that the volume of the hot air balloon increase due to the rise(increase) in temperature as the balloon is heated

Thus the expression is V \propto T

\frac {V}{T} = k where k is a constant  

When there is a change in the volume and temperature the expression will be

\frac {V_1}{T_1} = \frac {V_2}{T_2}

where V_1 and T_1 are the initial volume and initial temperature and V_2 and T_2 are the final volume and temperature.

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The expression of the theoretical yield (TY) in function of limiting reagent (LR) of a reaction is as follows: TY = ideal mole r
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<u>Answer:</u> The theoretical yield of acetanilide is 6.5 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For aniline:</u>

Given mass of aniline = 4.50\times 10^0=4.50g      (We know that:  10^0=1 )

Molar mass of aniline = 93.13 g/mol

Putting values in equation 1, we get:

\text{Moles of aniline}=\frac{4.50g}{93.13g/mol}=0.048mol

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To calculate the mass of acetic anhydride, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Volume of acetic anhydride = (1.25\times \text{Mass of aniline})=1.25\times 4.50=5.625mL

Density of acetic anhydride = 1.08 g/mL

Putting values in above equation:

1.08g/mL=\frac{\text{Mass of acetic anhydride}}{5.625mL}\\\\\text{Mass of acetic anhydride}=(1.08g/mL\times 5.625mL)=6.08g

Given mass of acetic anhydride = 6.08 g

Molar mass of acetic anhydride = 102.1 g/mol

Putting values in equation 1, we get:

\text{Moles of acetic anhydride}=\frac{6.08g}{102.1g/mol}=0.06mol

The chemical equation for the reaction of aniline and acetic anhydride follows:

C_6H_5NH_2+CH_3COOCOCH_3\rightarrow C_6H_5NHCOCH_3+CH_3COOH

By Stoichiometry of the reaction:

1 mole of aniline reacts with 1 mole of acetic anhydride

So, 0.048 moles of aniline will react with = \frac{1}{1}\times 0.048=0.048mol of acetic anhydride

As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.

Thus, aniline is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of aniline produces 1 mole of acetanilide

So, 0.048 moles of aniline will produce = \frac{1}{1}\times 0.048=0.048mol of acetanilide

Now, calculating the theoretical yield of acetanilide by using equation 1:

Moles of acetanilide = 0.048 moles

Molar mass of acetanilide = 135.17 g/mol

Putting values in equation 1, we get:

0.048mol=\frac{\text{Mass of acetanilide}}{135.17g/mol}\\\\\text{Mass of acetanilide}=(0.048mol\times 135.17g/mol)=6.5g

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