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
Activity 1: Ch. 13 New Material Clusters of 3 or 4 Vapor Pressure Problem: Glycerin (C3H803) is a nonvolatile nonelectrolyte with a density of 1.26 g/mL at 25 °C Calculate the vapor pressure at 25 °C of a solution made by adding 50.0 mL of glycerin to 500.0 mL of water. The vapor pressure of pure water at 25 °C is 23.8 torr, and its density is 1.00 g/mL. Equation Henry's Law Problem: Calculate the concentration of CO2 in a...
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.
Soft drinks “fizz” when opened. Calculate [CO2 ] when a drink is bottled (P = 4.5 atm), and after it’s opened. For CO2 in water kH = 3.4 x 10-2 M/atm. The partial P of CO2 in the atmosphere = 3.1 x 10-4 atm. explain?
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...
Hello guys I want help to solve those question please ! Calculate the mole fraction of phosphoric acid (H3PO4) in a 26.6% (by mass) aqueous solution. What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2 in 115 g of water? The molal freezing point depression constant for water is The concentration of CO2 in a soft drink bottled with a partial pressure of CO2 of 4.0 atm over the liquid at 25 °C...
Supose the gas above the soda in a bottle of soft drink is pure CO2 at a pressure of 4.5 atm. Calculate [CO2) at 25 C in mol/L at an elevation of 1100.0 m. Henry's law at 25°C is 0.03363 mol/(L*atm) A 0.151 M B 0.05 M C 0.084 M D 0.168 M E 0.118 M
What is the solubility of CO2 in a soft drink (which is mainly water) that was bottled under a CO2 pressure of 4.5 atm? Express your answer using two significant figures.
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.)...
A bottle of soda is opened and allowed to equilibrate at 25°C, at partial pressure= 0.95 6. atm. (Hint: refer to Henry's Law) a. (1pt) Calculate the concentration, in moles/L, of CO2 in the drink. Given ko02= 3.4 x 102 mol/(Latm) Ans. b.(Apt) If the partial pressure were higher, would you expect the concentration of carbon dioxide in the soda to be higher or lower than the answer to part a? Explain.