The solubility of a gas in a liquid increases with increasing pressure. To understand the above statement, consider a familiar example: cola. In cola and other soft drinks, carbon dioxide gas remains dissolved in solution as long as the can or bottle remains pressurized. As soon as the lid is opened and pressure is released, the CO2 gas is much less soluble and escapes into the air. Part B What pressure is required to achieve a CO2 concentration of 0.0480 mol L-1 at 20 C? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) The relationship between pressure and the solubility of a gas is expressed by Henry's law: Sgas = kH Pgas, Sgas Where is concentration in mol L, kH is the Henry's law constant in units of mol L bar, and Pgas is the pressure in bar. -1 Note: Since temperature also affects the solubility of a gas in a liquid, the Henry's law constant is specific to a particular gas at a particular temperature. b. X10n 1.1546 atm Submit Previous Answers X Incorrect; Try Again; One attempt remaining Part C At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20C to 25 C? Express your answer to four decimal places and include the appropriate units. View Available Hint(s) b X10" 3 7.2 10 mol Submit Previous Answers