Question

Calculate the concentration of Co2 in rainwater at 25C using Henry's law. Assume that the water...

Calculate the concentration of Co2 in rainwater at 25C using Henry's law. Assume that the water is saturated with air that contains 350 ppm of CO2. The Henry's law constant for CO2 is KH=3.4X10-2 MOL/L-ATM at 15C . Express the result in molarity and ppm. Calculate the concentration of NO in rainwater at 25 C that is in equlibrium with polluted air where the NO concentration is 10 ppm. The Henry's law constant for No is Kh=2x10-4 mol/l-atm at 25C .Express the result in molarity and ppb

Science   Chemistry   
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
CO2 dissolves in water to produce H2CO3 in the same way that SO2 produces H2SO3. (a)...
CO2 dissolves in water to produce H2CO3 in the same way that SO2 produces H2SO3. (a) Confirm by calculation that the pH of CO2-Saturated water at 25 degrees C is 5.6, given that the CO2 concentration in air is 365ppm. For carbon dioxide, the henry's law constant KH=3.4x10^-2M atm^-1 at 25 degrees C. The Ka for carbonic acid, H2CO3, is 4.5x10^-7. (b) Recalculate the pH for carbon dioxide concentration of 560ppm.
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)...
Henry's law constant for CO2 at 38oC is 2.28 x 10–3 mol/L\cdot⋅atm. Calculate the pH of...
Henry's law constant for CO2 at 38oC is 2.28 x 10–3 mol/L\cdot⋅atm. Calculate the pH of a solution of CO2 at 38oC in equilibrium with the gas at a partial pressure of 3.20 atm. Assume that all dissolved CO2 is in the form of carbonic acid (H2CO3). Ka1 = 4.3 x 10–7 and Ka2 = 5.6 x 10–11 for carbonic acid.
41. Henry's law constant for CO2 at 38°C is 2.28 ×10−3 mol / L · atm....
41. Henry's law constant for CO2 at 38°C is 2.28 ×10−3 mol / L · atm. Calculate the pH of a solution of CO2 at 38°C in equilibrium with the gas at a partial pressure of 3.25atm. A solution of formic acid (HCOOH) has a pH of 2.17. How many grams of formic acid are there in 100.0 mL of solution? g/100.0 mL
1. The atmospheric concentration of CO2 has exceeded 400 ppm for most of 2016. Water that...
1. The atmospheric concentration of CO2 has exceeded 400 ppm for most of 2016. Water that is in contact with air will absorb CO2 according to Henry’s Law: [CO2] = kCO2 ∙ PCO2 with kCO2 = 3.1×10–2M/atm at 25°C a) Use this information to calculate the molarity of CO2(aq) in rain water. Assume that the barometric pressure is 1 atm, the temperature is 25°C, and [CO2] is the equilibrium concentration. b) Calculate the pH of the rainwater assuming that all...
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...
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT