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?
Soft drinks “fizz” when opened. Calculate [CO2 ] when a drink is bottled (P = 4.5...
Calculate the concentration of CO2 in a soft drink that is bottled with a partial pressure of CO2 of 4.0 atm over the liquid at 25°C. The Henry's law constant for CO2 in water at this temperature is 3.1 X 10-2 mol/L.atm. O 0.12 M O 3.1M. 12.0M 0.31M 0.21M
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
Soft drinks are canned under 4.0 atm of CO2 (KH=3.3x10-2M/atm) and release the gas when opened. How many moles of CO2 are dissolved in a 355mL can of soda before it is opened? How many moles After is has gone flat here in CT where our atmospheric pressure is about 760torr regularly? And, using the ideal gas law, determine the volume in L the release CO2 would occupy at 1.00atm and 25C?
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.
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
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...
Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation CO2(gas)<------>CO2(aq) K=0.032 M*atm-1 The acid dissociation constants listed in most standard reference texts for carbonic acid actually apply to dissolved CO2. For a CO2 partial pressure of 3.1×10-4 atm in the atmosphere, what is the pH of water in equilibrium with the atmosphere?
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.
3) A soda can containing 355 mL of a carbonated soft drink is held at 3°C under 2.2 atm CO2 pressure. What is the concentration of CO2 in the soda, assuming that KH = 7.8 x 10-2 M/atm? 4) When 0.64 g of adrenaline is dissolved in 36.0 g C6H6 (Kf = 5.12 °C), the freezing point is lowered by 0.50 °C. Determine the molar mass of adrenaline. 5) Carbon tetrachloride, and important industrial solvent is made from methane via...
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.