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
Calculate the concentration in units of mg/L for oxygen dissolved in 1050.0 mL of water at...
What is the concentration (in mg/L) of dissolved O, in blood (or water) at this partial pressure and a normal body temperature of 37°C? The solubility of O2 in water at 37°C and 1atm partial pressure is 1.93 x 10 mol/L Express your answer using two significant figures. O AXO ? 0] mg/L Submit Request Answer
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.41 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. 96.3 mg 49.4 mg 63.2 mg 48.2 mg
26 Calculate the equilibrium concentration of dissolved oxygen in 15°C water at 1 atm, and again at 2,000 m elevation. Suppose the gas above the soda in a bottle of soft drink is pure CO2 at a pressure of 2 atm. Calculate (CO2) at 25°C. 27
Dissolved Oxygen in Water Sample Question 1. Calculate the dissolved oxygen for 300 ml sample of water that was analyzed using Winkler method with azide modification. The sample were titrated against standard 0.025 N of sodium thiosulphate, and the required volume of sodium thiosulphate to reach the colorless endpoint was 13.5ml. Question 2. A student conducted an experiment to measure the biochemical oxygen demand for 400 ml of waste water. She diluted the sample by adding 600 ml of oxygen...
the equilibrium concentration of dissolved oxygen jn mg/L in Lake Titicaca. The elevation is 3.850 m (atmospheric pressure = 0.62 atm)? Assume T-20 °C and K 0.62 atm)? Assume T-20 °C and Kn730 atm-L/mol. What would the concentration be with the same temperature at sea level? Explain the significance of this equation for a) developing and b) developed countries: 1 - (P)(A)(T)
Calculate the masses of oxygen and nitrogen that are dissolved in 7.0 L of aqueous solution in equilibrium with air at 25 °C and 760 Torr. Assume that air is 21% oxygen and 78% nitrogen by volume. Henry's law constants for gases in water at 25 °C Gas He kh (bar · M-1) 2.7 x 103 1.6 x 103 7.9 x 102 29 mass: mg 02 CO2 HS mass: mg N2 10.
g. What is the expected concentration of oxygen in open bodies water like lakes and rivers that are in contact with the atmosphere at 25 °C? What is the mass of dissolved O2 in 1 iter of water? Assume partial pressure of O2 in atmosphere is 0.22 bar and use Henry's Law constant K.30x102 mol(m3 kPa) for oxygen in water.
I'm working on a prelab titled: Analysis of Water for Dissolved Oxygen. The question is: Calculate the concentration in mg/L (ppm) of a solution that is 4*10^-3M in O2, assuming a density of 1g/mL for the solution. I'm not sure if I provided all of the information needed, seeing as how I don't entirely understand the question. Any help would be appreciated. Thank you.
Hydrogen gas, H2, and oxygen gas, O2, can be reacted to form liquid water. If 2.00 g hydrogen gas and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25 °C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question. Total gas pressure:
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...