Calculate the theoretical oxygen demand for a 130 mg/L aqueous solution of lactic acid (C3H6O3).
Calculate the equilibrium concentration of dissolved oxygen in 25°C water at sea level (p = 1.00 atm), and again at 4000 m elevation in 5°C water. [Use the exponential p vs. z equation, not the empirical formula.]
Calculate the theoretical oxygen demand for a 130 mg/L aqueous solution of lactic acid (C3H6O3). Calculate...
Calculate the equilibrium concentration of dissolved oxygen in 25°C water at sea level (p = 1.00 atm), and again at 4000 m elevation in 5°C water. [Use the exponential p vs. z equation provided in the lectures, not the empirical formula given in the textbook.] P(z)=P(O)exp(-z/H)
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)
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
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.
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 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
Theoretical Oxygen Demand (ThOD) Calculations Calculate the ThOD of 120 mg/L wastewater (CaHrO2N) assuming the following stoichiometry is valid. Answer: ThoD 257.7 3. mg/L)
2. Given ky of 3.4 x 10-2 [mol L atm'), calculate the dissolved aqueous concentration of CO2 that would be at equilibrium with current CO2 concentrations in the atmosphere. (2 pts) The other reactions above are similarly associated with equilibrium constants: K, - [H.CO] CO2/01)] , [H][HCO3] K - TH.CO;] H][co;] THCO3] where K, = 1.7x10-3, K, = 2.5x10+ , and K. = 4.7 x 10-11 3. Knowing the reaction constants above, calculate the pH of water that is in...
Benzene: Kow: 1.99 Aqueous Solubility: 2000 mg/L Vapor Pressure: 75 mmHg Spill description: A truck containing 5000 grams of your assigned chemical has spilled into a closed lake with the following dimensions: 100 meters long, 100 meters wide, and 1 meter deep. What is the concentration of your chemical (in grams per liter) in the lake assuming it quickly reaches equilibrium and lake is filled to the brim with water? This is not something we covered specifically in class; however,...
A chemistry teacher needs to make 2.30 L of a potassium chloride solution for an experimen The concentration of the required solution is 3.10 M. How many grams of KCI will she need to use? 0 7.13 g KCI 0 231 g KCI O 532 g KCI 0.0956 g KCI What is the equation for the ion product constant of water at 25 °C? Kw [H,0+][OH-] [H,O] = 1.00 x 10-14 Kw [H,0+1 [OH-] = 1.00 x 10-14 Kw =...