Question

# Henry's Law states that the quantity of a gas that will dissolve in a liquid is...

Henry's Law states that the quantity of a gas that will dissolve in a liquid is proportional to the partial pressure of the gas and its solubility coefficient (its physical or chemical attraction for water), at a given temperature. Henry's Law: The volume of a gas (Vx) dissolved in a liter of water is Vx = (pX)*(SC), where pX is the partial pressure in atmospheres and SC is the solubility coefficient.

a) At 1 atm and 37 degrees Celsius, the solubility coefficient for oxygen is 0.024 ml O2/ml H2O. How much oxygen can dissolve in a liter of water at 37 degrees Celsius if the partial pressure of oxygen is 85 mm Hg =

b) At 1 atm and 20 degrees Celsius, the solubility coefficient for Carbon dioxide is 0.88 ml CO2/ml H2O at one atmosphere. How much CO2 can dissolve in a liter of water at 20 degrees Celsius if the partial pressure of CO2 is 38 mm Hg?

a)

Partial pressure $P_{O2}=\frac{85 \ mm \ Hg}{760 \ mm \ Hg}=0.1118 \ atm$

$V_{O2}=P_{O2} \times SC$

$V_{O2}=0.1118 \ atm \times \frac{0.024 \ ml \ O_2}{ml \ H_2O}$

$V_{O2}= \frac{ 0.002684 \ ml \ O_2}{ml \ H_2O}$

For 1 L (1000 mL of water)

$V_{O2}= \frac{ 0.002684 \ ml \ O_2}{ml \ H_2O} \times \frac{ 1000 \ mL \ H_2O}{ 1 \ L \ H_2O}$

$V_{O2}= \frac{ 2.68 \ ml \ O_2}{L \ H_2O}$

b)

Partial pressure $P_{CO2}=\frac{38 \ mm \ Hg}{760 \ mm \ Hg}=0.05 \ atm$

$V_{CO2}=P_{CO2} \times SC$

$V_{CO2}=0.05 \ atm \times \frac{0.88 \ ml \ CO_2}{ml \ H_2O}$

$V_{CO2}= \frac{ 0.044 \ ml \ CO_2}{ml \ H_2O}$

For 1 L (1000 mL of water)

$V_{CO2}= \frac{ 0.044 \ ml \ CO_2}{ml \ H_2O} \times \frac{ 1000 \ mL \ H_2O}{ 1 \ L \ H_2O}$

$V_{CO2}= \frac{ 44 \ ml \ CO_2}{L \ H_2O}$

#### Earn Coins

Coins can be redeemed for fabulous gifts.

Similar Homework Help Questions
• ### 9. Henry's Law states that the quantity of a gas that will dissolve in a liquid...

9. Henry's Law states that the quantity of a gas that will dissolve in a liquid is proportional to the partial pressure of the gas and its solubility coefficient (its physical or chemical attraction for water), at a given temperature a) Henry's Law: The volume of a gas (Vx) dissolved in a liter of water is Vx= (p3)*(SC) where pX is the partial pressure in atmospheres and SC is the solubility coefficient b) At one atmosphere and 37 degrees Celsius,...

• ### please help I don't understand Using Henry's Law to calculate the solubility of a gas At 25.0 °C the Henry'...

please help I don't understand Using Henry's Law to calculate the solubility of a gas At 25.0 °C the Henry's Law constant for hydrogen sulfide (HS gas in water is 0.087 M/atm grams of HS gas that can be dissolved in 150. mL of water at 25.0 °C and a H,S partial pressure of 1.53 atm Calculate the mass Be sure your answer has the correct number of significant digits. X Check Explanation Using Henry's Law to calculate the solubility...

• ### TUTOR Henry's Law Oxygen gas has a Henry's law constant of 1.66x10 M/mmHg at 25.0 °C...

TUTOR Henry's Law Oxygen gas has a Henry's law constant of 1.66x10 M/mmHg at 25.0 °C when dissolving in water. If the total pressure of gas (O2 gas plus water vapor) over water is 1.00 atm, what is the concentration of O2 in the water in grams per milliliter? Pressure of the water vapor at 25.0 °C-23.8 mmHg. g/mL

• ### need help with part b please Henry's Law Henry's Law states that the solubility of a...

need help with part b please Henry's Law Henry's Law states that the solubility of a gas in a liquid (at a constant temperature) is entirely dependent on the partial pressure of that gas above the liquid. Increasing the pressure of increases the presence of that gas in the solution. We have talked about soda, carbonated with CO). These sodas are carbonated by placing the soda under a high COpressure Considering Henry's Law for gas solubility, consider the top of...

• ### Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and...

Use Henry's law and the solubilities given below to calculate the total volume of nitrogen and oxygen gas that should bubble out of 1.6 L of water upon warming from 25 ∘C to 50 ∘C. Assume that the water is initially saturated with nitrogen and oxygen gas at 25 ∘C and a total pressure of 1.0 atm. Assume that the gas bubbles out at a temperature of 50 ∘C. The solubility of oxygen gas at 50 ∘C is 27.8 mg/L...

• ### The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L • atm) at...

The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L • atm) at 25°C. What is the solubility of methyl bromide in water at 25°C and at a partial pressure of 270. mm Hg?

• ### If 136.2 mL of water is shaken with oxygen gas at 3.0 atm, it will dissolve...

If 136.2 mL of water is shaken with oxygen gas at 3.0 atm, it will dissolve 0.0036 g O2. Estimate the Henry's law constant for the oxygen gas in water in units of g mL-1atm-1.

• ### Henry's Law Example Sgas = kw X Pgas • At 20°C ky for argon (gas) in...

Henry's Law Example Sgas = kw X Pgas • At 20°C ky for argon (gas) in water is 1.64 x 10-3 molal/atm. How many grams of argon will dissolve in 500 g of water (d = 1.0 g/mL) if the pressure of argon above the solution is 2.5 atm?

• ### Henry’s law states that the solubility of a gas is directly proportional to the partial pressure...

Henry’s law states that the solubility of a gas is directly proportional to the partial pressure of the gas if the temperature is constant. Hyperbaric chambers, which provide high pressures (up to 6 atm) of either air or pure oxygen, are used to treat a variety of conditions, ranging from decompression sickness in deep-sea divers to carbon monoxide poisoning. Look up the Henry’s Law Constant (kH) for N2, O2, and CO2 in the textbook. a) Calculate the solubility (concentration in...

• ### Carbonated beverages are manufactured to dissolve carbon dioxide gas at high pressure that is released when...

Carbonated beverages are manufactured to dissolve carbon dioxide gas at high pressure that is released when the can is opened so that the beverage is more refreshing to the consumer. How many grams of dissolved carbon dioxide is in a 355mL can of soda at 20 degrees Celcius if the manufacturer used a pressure of 2.4 atm of CO2 to carbonate the pop? The Henry's law constant for carbon dioxide dissolving in water is 3.5*10-2 mol/L*atm at 20 degrees Celcius.