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GarryVolchara [31]
2 years ago
15

When Logan opens a new bottle of carbonated beverage, the sudden release of pressure causes the beverage to bubble up and overfl

ow. What could Logan do in the future to prevent the next bottle from overflowing when he opens it
Chemistry
1 answer:
AfilCa [17]2 years ago
6 0

Answer:

When Logan opens a new bottle of carbonated beverage, the sudden release of pressure causes the beverage to bubble up and overflow. What could Logan do in the future to prevent the next bottle from overflowing when he opens it.

Explanation:

This is an application of Boyle's law.

According to Boyle's law:

the volume of a fixed amount of gas is inversely proportional to its pressure at a constant temperature.

V  \alpha   \frac{1}{P}

So, if pressure reduces all of a sudden, the volume increases and this causes an overflow of the beverage from the bottle.

To avoid this situation, the pressure inside the bottle should not be released at once. The bottle cap should be opened slowly in such a way that opens a little and then close again open a little and then close like that many times if we do, then pressure inside the bottle goes slowly then, the volume will not increase all of a sudden.

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Given mass of testosterone = 7.752 g

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Putting values in equation 1, we get:

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Given mass of diethyl ether = 208.0 g

Molar mass of diethyl ether = 74.12 g/mol

Putting values in equation 1, we get:

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The formula for relative lowering of vapor pressure will be:

\frac{p^o-p_s}{p^o}=i\times \chi_{\text{solute}}

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p^o = vapor pressure of solvent (diethyl ether) = 463.57 mmHg

p^s = vapor pressure of the solution = ?

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\chi_{\text{solute}} = mole fraction of solute (testosterone) = 0.0095

Putting values in above equation, we get:

\frac{463.57-p^s}{463.57}=1\times 0.0095\\\\p^s=459.17mmHg

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