g. What is the expected concentration of oxygen in open bodies water like lakes and rivers...
Calculate the solubility of oxygen in water at a partial pressure of O2 of 343 torr at 25°C. The Henry's Law constant for oxygen in water is 1.28 x 10 mol/(atm L). mol/L
6.) The solubility of CO2 (g) in water is 3.2 x 102 M at 25.0 °C and 1.0 atm pressure. a.) What is the Henry's Law constant for CO2 (g)? Cg = k P, ; Cg = concentration in M; k = Henry's Law constant in mol L atm*'; P. = pressure in atm. 3.2 x 10-2 M=k (1.0 atm) (3.2 x 10-2 M)/(1.0 atm) = k = 3.2 x 10-2 M/atm = 3.2 x 10-2 mol L atm" b.)...
1.The solubility of O2 in water is 0.590 g/L at an oxygen pressure of around 15.5 atm. What is the Henry's law constant for O2 (in units of mol/L
100 mL of air is in contact with 1L of pure water in a closed vessel at 10°c. If the water is initially oxygen free, once equilibrium has been reached, what is the concentration of oxygen in the water and the partial pressure of oxygen in the air once equilibrium has been reached? Assume no volatility due to water. The Henry's constant for oxygen is 588 atm.L/mol at 10°C. What other assumptions do you make in performing this calculation? Note...
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...
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
Question 3 The current partial pressure of Co, in the Earth's atmosphere is 3.9 · 104 atm. If the Henry's law constant is 2.3 · 10M/atm, calculate the equilibrium concentration of dissolved CO2 in bodies of water. Incorrect 0.00 points out of 0.30 p Flag question Select one: A. 1.7 x 10PM © B. 59 M X C. 9.0 x 100M O D. 9.0 x 100M
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...
1- A person performing ambient pressure diving descends to a depth of 30.0 m. a) Calculate the total pressure exerted on the diver by the atmosphere and the surrounding water. (2 pts) b) Assuming the pressure of the gas mixture inhaled by the diver is adjusted to equal the ambient pressure at that depth, calculate the concentration of oxygen dissolved in the diver's tissues (mol/L). Assume the gas mixture is 21% oxygen. Assume the tissue fluid can be treated as...
Calculate the concentration in units of mg/L for oxygen dissolved in 1050.0 mL of water at 25 °C, if the partial pressure of O2 in gas phase in equilibrium with the water is 238.1 mm Hg. Assume the density of water =1 g/mL