The partial pressure of CO2 gas above the liquid in a carbonated drink is 0.45 atm. Assuming that the Henry's law constant for CO2 in the drink is that same as that in water, 3.7 x 10-2 mol/L atm, calculate the solubility of carbon dioxide in this drink. Give your answer to 3 decimal places.

Find the molal freezing point

nestion 8 When carbonating fruit, the initial partial pressure of CO2 is 6.56 x 104 atm, resulting in a concentration of 4.56 x 10¬³ M. If the partial pressure of CO, rises to 3.01 atm, what is the new concentration of CO2 dissolved in M? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) A Moving to another question will save this response. Question 8 of 29 44. %23 4. 5 8. delete Q E R т Y AI S D G L H F K C alt alt option command command option

Calculate the vapor pressure, in mmHg of a solution made by dissolving 285 g of glucose (molar mass 180.2 g/mol) in 404 mL of water at 40°C. The vapor pressure of pure water at 40°C is 55.32 mmHg. The density of pure water is 1.00 g/mL. Report your answer to four significant figures. Do not include units in your answer

A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.

A student dissolves 8.0 g of phenol (CH₂OH) in 125. mL of a solvent with a density of 1.06 g/mL. The student notices that the volume of the solvent does not change when the phenol dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity molality = x10 DO 0x0

A student dissolves 14. g of sucrose (C,,H,,0,1) in 450. mL of a solvent with a density of 0.85 g/mL. The student notices that the volume of the solvent 22 does not change when the sucrose dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity = | x10 molality %3D Continue Submit O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center MacBook Air 20 888 DD F3 F4 F5 F6 F7 F8 34 00

A student dissolves 8.3 of phenol (CH,OH) in 325. mL of a solvent with a density of 1.12 g/mL. The student notices that the volume of the solvent does not change when the phenol dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. molarity x10 molality 미

The solubility in water of ionic compound x is measured and found to be 0.799 at 20. °C. Calculate the volume of a saturated solution of x in water that would contain 390. mg of x at this temperature. Be sure your answer has the correct unit symbol and number of significant digits. 0 g mL x10 3 00 8

The normal freezing point of a certain liquid X is 5.20 °C, but when 41. g of urea (CH,N,O) are dissolved in 750. g of X the solution freezes at 2.5 °C instead. Use this information to calculate the molal freezing point depression constant K, of Х. Round your answer to 2 significant digits. °C·kg x10 K, = 0 mol