Question

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 2.0 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 at an oxygen pressure of 1.00 atm. The solubility of nitrogen gas at 50 ∘C is 14.6 mg/L at a nitrogen pressure of 1.00 atm. Assume that the air above the water contains an oxygen partial pressure of 0.21 atm and a nitrogen partial pressure of 0.78 atm. (please include the full answer)

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Using Raoult's law for water and Henry's law for nitrogen, calculate the pressure and gas-phase composition...
Using Raoult's law for water and Henry's law for nitrogen, calculate the pressure and gas-phase composition (mole fractions) in a system containing a liquid that is 1.200 mole% N2 and 98.80 mole% water in equilibrium with nitrogen gas and water vapor at 50.0°C. The Henry's law constant for nitrogen in water is recommended by NIST to be well represented by kH = 0.000625 exp[1300 (1/T – 1/298.15)] mol N2 / (kg H2O bar), where T is measured in Kelvin a)...
The solubility of oxygen, O2, in water is 7.20 ✕ 10−4 mol/L at 0°C when the...
The solubility of oxygen, O2, in water is 7.20 ✕ 10−4 mol/L at 0°C when the nitrogen pressure above water is 0.554 atm. Calculate the solubility of oxygen in water when the partial pressure of oxygen above water is 1.083 atm at 0°C? The Henry's Law constant for oxygen is 1.30 ✕ 10−3 mol/ L atm.
A gas mixture of nitrogen and oxygen having a total pressure of 2.50 atm is above...
A gas mixture of nitrogen and oxygen having a total pressure of 2.50 atm is above 2.0 L of water at 25 °C. The water has 51.3 mg of nitrogen dissolved in it. What is the molar composition of nitrogen and oxygen in the gas mixture? The Henry’s constants for N2 and O2 in water at 25 °C are 6.1×10–4 M/atm and 1.3×10–3 M/atm, respectively.
The Henry's law constant for O2 in water at 25 °C is 1.25 × 10-5 mol...
The Henry's law constant for O2 in water at 25 °C is 1.25 × 10-5 mol L-1 kPa-1, and the solubility is 1.5 × 10-3 mol L-1. What is the partial pressure of O2 under these conditions?
a) Use Henry's law to determine the molar solubility of helium at a pressure of 1.8...
a) Use Henry's law to determine the molar solubility of helium at a pressure of 1.8 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. Express your answer using two significant figures. b) An aqueous solution containing 36.7 g  of an unknown molecular (non-electrolyte) compound in 160.0 g of water was found to have a freezing point of -1.5 ∘C. Calculate the molar mass of the unknown compound. Express your answer using two...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. 2) A 2.800×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.2 mL...
Exercise 11.76 A mixture of helium, nitrogen, and oxygen has a total pressure of 755 mmHg...
Exercise 11.76 A mixture of helium, nitrogen, and oxygen has a total pressure of 755 mmHg . The partial pressures of helium and nitrogen are 241 mmHg and 194 mmHg , respectively. Part A What is the partial pressure of oxygen in the mixture? ​Part B The hydrogen gas formed in a chemical reaction is collected over water at 30 ∘C at a total pressure of 730 mmHg . What is the partial pressure of the hydrogen gas collected in...
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm...
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is5.6 × 10−4 mol/L. A deep-sea diver breathes compressed air with the partial pressure of N2 equal to 5.0 atm. Assume that the total volume of blood in the body is 5.2 L. Calculate the amount of N2 gas released (in liters at 37°C and 1.00 atm) when the diver returns to the surface of the water, where the partial pressure of N2 is...
37)Into a 15.00-liter container at 25°C are placed 1.00 moles of O2 gas and 3.00 moles...
37)Into a 15.00-liter container at 25°C are placed 1.00 moles of O2 gas and 3.00 moles of solid C (graphite). If the carbon and oxygen react completely to form CO(g), what will be the final pressure in the container at 25°C? a) 0.274 atm b) 1.00 atm c) 4.89 atm d) 1.63 atm e) 3.26 atm 39) N2 (g) + 3H2 (g) 2NH3 (g). If a 3.4 L flask is first charged with 1.2 atm of nitrogen, then hydrogen is...
A weather balloon contains 222 L of He gas at 20. °C and 760. mmHg. What...
A weather balloon contains 222 L of He gas at 20. °C and 760. mmHg. What is the volume of the balloon when it ascends to an altitude where the temperature is -40. °C and 540. mmHg? 1 What volume does 12.5 g of Ar gas at a pressure of 1.05 atm and a temperature of 322 K occupy? Would the volume be different if the sample were 12.5 g of He gas under the same conditions? How many moles...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT