Chemistry, 25.08.2019 04:30 artursino

Sort each of the following events based on whether the solubility of the indicated gas will increase, decrease, or stay the same. each phrase specifies the gas involved and the change in its environment.
1. the temperature is increased 2.the partial pressure of an anesthetic gas is increased
3.o2: temperature of a body when water rises 4. the pressure of a gas over a solvent is increased
5. air in blood: a diver descends 10m and pressure increase by 1 am
me and tell me which ones gas solubility increase, decrease or the gas stays the same.
i got 1 and 5 for decrease. the 2, 3, 4 for increase.

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Answer from: Taylor129

1. The solubility of the anesthetic gas $\boxed{{\text{decreases}}}$ if the temperature is increased.

2. The solubility of the anesthetic gas $\boxed{{\text{increases}}}$ if its partial pressure is increased.

3. The solubility of the oxygen $\boxed{{\text{decreases}}}$ if the temperature of the body is increased.

4. The solubility of oxygen $\boxed{{\text{increases}}}$ if its pressure over the solvent is increased.

5. The solubility of air in blood $\boxed{{\text{increases}}}$ if diver descends $10\;{\text{m}}$ and the pressure is increased by ${\text{1}}\;{\text{atm}}$ .

Further Explanation:

The chemical property of any substance that makes it capable to dissolve in other substances is called solubility. It is measured in terms of the maximum amount of solute that can be dissolved in the given amount of solvent.

Solubility is directly related to the intermolecular forces. Moreover, temperature and pressure are two other factors that influence the solubility of the gas.

There exist weak intermolecular forces between the gas molecules. With the increase in the temperature, the average kinetic energy also speeds up due to which the molecules start vibrating about their mean positions. This results in overcoming of the weak forces and the molecules re-enter into the gas phase. So solubility decreases with the increase in temperature.

The law that governs the relationship of gas solubility with its partial pressure is Henry’s Law. It states that the solubility $\left( {{{\text{S}}_{{\text{gas}}}}} \right)$ is directly proportional to the partial pressure $\left( {{{\text{P}}_{{\text{gas}}}}} \right)$ of the gas. If the gas has high partial pressure, it will have a higher solubility and vice-versa.

Mathematically, ${{\mathbf{S}}_{{\mathbf{gas}}}} \propto {{\mathbf{P}}_{{\mathbf{gas}}}}$

We incorporate a proportionality constant in order to remove the sign of proportionality. That constant is known as Henry’s constant, represented by ${{\mathbf{k}}_{\mathbf{H}}}$ .

So Henry’s Law becomes ${{\mathbf{S}}_{{\mathbf{gas}}}} = {{\mathbf{k}}_{\mathbf{H}}}{\mathbf{ \times }}\;{{\mathbf{P}}_{{\mathbf{gas}}}}$

1. As we know, the solubility of gas is inversely proportional to the temperature. So if the temperature of anesthetic gas is increased, its solubility decreases.

2. According to Henry’s Law, the solubility of gas is directly proportional to the partial pressure of the gas. So the solubility of anesthetic gas also increases with the increase in its partial pressure.

3. As we know, the solubility of gas is inversely proportional to the temperature. So if the temperature of the body is increased, the solubility of oxygen decreases.

4. According to Henry’s Law, the solubility of gas is directly proportional to the partial pressure of the gas. So the solubility of oxygen also increases with the increase in its partial pressure.

5. As the diver descends $10\;{\text{m}}$ and the pressure is increased by $1\;{\text{atm}}$ , the solubility of gas increases in accordance with Henry’s Law.

Learn more:

1. Statement about subatomic particle:

2. The energy of a photon in light:

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Solutions

Keywords: solubility, gas, increase, decrease, temperature, partial pressure, diver, air, change, environment, oxygen, blood, Henry's Law, anesthetic gas.

Answer from: Quest

The answer for this question is d. none of these

Answer from: Quest

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