Use this value (401.7 ppm CO2) to calculate the molar concentration (i.e., in units of moles/L...
Use this value (401.7 ppm CO2) to calculate the molar concentration (i.e., in units of moles/L or M) of dissolved CO2 in rainwater in equilibrium with the atmosphere at 25 oC. The Henry’s Law constant for CO2 at 25 oC is 10-1.5 mol L-1 atm-1.
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Use this value (401.7 ppm CO2) to calculate the molar
concentration (i.e., in units of moles/L...
b) The current (Year 2017) atmospheric CO2 concentration is 370 ppm. It is estimated that if...
b) The current (Year 2017) atmospheric CO2 concentration is 370 ppm. It is estimated that if we continue to exploit the world’s fossil fuel reserves at the same rate, the atmospheric CO2 concentration will reach 1,100 ppm in Year 2400 (Williams, 2001). Justify your answer in (1) quantitatively by calculating the pHs when CO2 concentrations are 370 ppm (Year 2017) and 1,100 ppm (Year 2400), respectively. Assuming: I. Pure water is in equilibrium with CO2 at 25oC. II. Water vapor...
Calculate the concentration of CO2 in a soft drink that is bottled with a partial pressure...
Calculate the concentration of CO2 in a soft drink that is bottled with a partial pressure of CO2 of 5 atm over the liquid at 25 °C. The Henry’s Law constant for CO2 in water at this temperature is 3.12 ´ 10–2 mol L–1 atm–1. 1. 0.16 2. 0.26 3. 1.26 4. 1.16 5. 0.56
The concentration of dissolved CO2 gas in seawater is 5.00 x 10^–3 mol L–1 . The...
The concentration of dissolved CO2 gas in seawater is 5.00 x 10^–3 mol L–1 . The Henry’s law constant for CO2 at 298 K is 3.13 x 10^–7 mol L–1 Pa–1 . Calculate the partial pressure of carbon dioxide gas in the atmosphere above the ocean. (A) 16.0 kPa (B) 6.30 x 10–5 Pa (C) 1.57 x 10–9 Pa (D) 6.30 x 108 kPa
Current CO2 composition in air is about 380 ppm (mol/mol). What is [CO2 (aq)] dissolved in...
Current CO2 composition in air is about 380 ppm (mol/mol). What is [CO2 (aq)] dissolved in pure water, given Henry’s constant 0.034 M/atm. Assume air pressure is 1.00 atm. I got 1.29x10-5 M when I did my calculations.
1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What...
1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm? 2.The carbon dioxide concentration in a bottle of club soda is 0.12 mol L-1 at 25 °C. What is the pressure of carbon dioxide in the headspace? The Henry’s Law constant for CO2 at...
Calculate the concentration of CO2 in water at 25°C when the pressure of CO2 over the...
Calculate the concentration of CO2 in water at 25°C when the pressure of CO2 over the solution is 6.1 atm. At 25°C, the Henry's law constant for CO2 in water is 3.1 × 10−2 mol/L · atm.
1- At 25 oC the Henry’s Law constant for carbon dioxide (CO2) dissolved in water is...
1- At 25 oC the Henry’s Law constant for carbon dioxide (CO2) dissolved in water is 3.3 x 10-2 mol/L atm. Calculate the solubility of CO2 if the partial pressure of carbon dioxide gas inside a bottle of Fizzy Cola Drink is 6 atm at 25 C 2- Using Raoult’s Law, calculate vapor pressure lowering, DP = C · Po, when 14.0 mL of glycerol (C3H8O3) is added to 496.0 mL of water at 50.0 C. The density of glycerol...
Enter your answer in the provided box. The formula that governs the concentration of gas dissolved...
Enter your answer in the provided box. The formula that governs the concentration of gas dissolved in a solvent based on its pressure is given by Henry's Law: C= KP Where: C = solubility of a gas at a fixed temperature (in mol/L, M) k= Henry's Law constant (in units of mol/L • atm) P = partial pressure of the gas (in units of atm) How many grams of carbon dioxide gas is dissolved in a 290-ml can of cola...
Question 13 Calculate the amount of dissolved oxygen (ppm 02) using the following data: • Sample...
Question 13 Calculate the amount of dissolved oxygen (ppm 02) using the following data: • Sample volume (mL) = 224.893 • Buret Reading, initial (mL) = 3.581 • Buret Reading, final (mL) = 18.25 • Volume of Na2S203 dispensed (mL) = • Average molar concentration of Na2S203 (mol/L) = 0.0219 • Moles of Na2S203 dispensed (mol) = • Moles of 13° reduced by S2032-(mol) = • Moles of O2 (mol) = • Mass of O2 (mg) • Dissolved oxygen, ppm...
Calculate the concentration of CO 2 in orange soda that was bottled (at a certain temperature)...
Calculate the concentration of CO 2 in orange soda that was bottled (at a certain temperature) with a partial pressure of CO 2 of 3.15 atm over the liquid. At that temperature, the Henry's law constant, k, for CO 2 is 3.05 x 10 -2 mol/L atm. (i.e., 3.05 x 10 -2 M/atm) 14.0 M 8.12 M 2.74 M 6.63 x 10 -3 M 0.0961 M 23.8 M 11.9 M 7.93 x 10 -1 M 2. What is the mole fraction of sucrose when...
Enter your answer in the provided box. The formula that governs the concentration of gas dissolved in a solvent based on its pressure is given by Henry's Law: C= KP Where: C = solubility of a gas at a fixed temperature (in mol/L, M) k= Henry's Law constant (in units of mol/L • atm) P = partial pressure of the gas (in units of atm) How many grams of carbon dioxide gas is dissolved in a 290-ml can of cola...
Question 13 Calculate the amount of dissolved oxygen (ppm 02) using the following data: • Sample volume (mL) = 224.893 • Buret Reading, initial (mL) = 3.581 • Buret Reading, final (mL) = 18.25 • Volume of Na2S203 dispensed (mL) = • Average molar concentration of Na2S203 (mol/L) = 0.0219 • Moles of Na2S203 dispensed (mol) = • Moles of 13° reduced by S2032-(mol) = • Moles of O2 (mol) = • Mass of O2 (mg) • Dissolved oxygen, ppm...
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