Which of the following processes has an increase in entropy?

2 answers:

7 0

Entropy is defined as "randomness," so having that in mind, the process which has an increase in entropy is A. boiling a pot of water because when you boil water, the molecules space out and become gas.

marishachu [46]2 years ago

7 0

Answer: Option (A) is the correct answer.

Explanation:

Entropy is defined as the degree of randomness. This means that more is the temperature provided to a system more rapidly its molecules will move.

Therefore, molecules of water in a boiling pot will show maximum randomness. As a result, boiling a pot of water has an increase in entropy.

Thus, we can conclude that out of the given options processes that has an increase in entropy is boiling pot of water.

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Calculate the osmotic pressure associated with 50.0 g of an enzyme of molecular weight 98 g/mol dissolved in water to give 2600

andrew-mc [135]

Answer:

π = 4,882 atm

Explanation:

To calculate the osmotic pressure (π), the Van´t Hoff equation must be used, which is:

π x V = n x R x T

Where:

• π: Osmotic pressure, which is the difference between the levels of the solution and the pure solvent through a semipermeable membrane, which allows the passage of the solvent but not the solute

• V: Volume of the solution, in liters unit

• n: Number of moles of solute

• R: Constant of ideal gases, equal to 0.08206 L.atm / mol.K

• T: Absolute temperature, in Kelvin degrees

With the data you provide you can calculate the osmotic pressure by clearing it from the equation, we would be equal to:

π = (n x R x T) / V

However, all data must first be converted to the corresponding units in order to replace the values in the equation.

Solution volume ⇒ go from mL to L: 

1000 mL of solution ____ 1 L

2600 mL of solution _____ X = 2.6 L

Calculation: 2600 mL x 1 L / 1000 mL = 2.6 L

Temperature ⇒ Go from ° C to K 