Compound methanol ethanol propanol C3H;OH butanol CH3OH C2H5OH C4H9OH Vapor Pressure at 20 °C 11.9 kPa 5.95 kPa 2.67 kPa 0.56 kPa

The average osmotic pressure of blood is 7.7 atm at 25 °C. What molarity of glucose 1C6H12O62 will be isotonic with blood?

A student was instructed to determine the molecular weight of an unknown white powder. He remembered that one way to do this is by exploiting the colligative properties of solution. After a simple conductivity test, he found that an aqueous solution of the sample is not conductive. He dissolved 22.87 grams of the unknown sample in 0.500 kg of water. He found that the boiling point of the resulting solution was 100.13 °C under normal atmospheric conditions. Given: K, of water is 0.512 °C/m a. Calculate the molality of the resulting solution. b. How many moles of the sample did he dissolve to perform the experiment? c. What is the molecular weight of the unknown sample?

5 .  If 40.2g NaCl are mixed into water and the total mass is 389g, what is the CHANGE in boiling if Kb= 0.52C/M (molal)?    Assume NaCl does not dissociate in solution.

A soln is made of 2 volatile components: toluene and benzene. At 60 degrees Celsius, the vapor pressure of benzene (C6H6) is 396mmHg and the vapor pressure of toluene (C7H8) is 1.40*102mmHg. The soln has 0.25 moles benzene and 0.50 moles toluene. Calculate the total pressure of the soln.

Compound XY is an ionic compound that dissociates as it dissolves in water. The lattice energy of XY is -594.4 kJ mol1. The hydration energy of its ions is -626.2 kJ mol-1. Write the thermochemical equations for the two steps in the formation of a solution of XY in water. Draw an enthalpy diagram for the formation of this solution. What is the net AH for the formation of a solution of XY? i kJ mol-1

15 g of an unknown molecular substance was dissolved in 450 g of water. The resulting solution freezes at – 0.34 °C. What is the molar mass of the substance? (Kf for water = 1.86 K kg mol-1)

A solution of ethanol (CH,CH,OH) and water that is 90.% ethanol by mass is boiling at 81.9 °C. The vapor is collected and cooled until it condenses to form a new solution. Calculate the percent by mass of ethanol in the new solution. Here's some data you may need: normal vapor pressure density boiling point at 81.9 °C g 0.79 mL ethanol 78. °C 865. torr 100. °C 1.00 mL 389. torr water Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution and vapor above it are ideal. ?

bmitted The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 12.10 grams of chromium(II) bromide, CrBr₂ (211.8 g/mol), in 241.5 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3CH₂OH CHCI 3 C6H6 Diethyl ether CH3CH₂CH₂CH3 The molality of the solution is The boiling point of the solution is Submit Answer Retry Entire Group Kb (°C/m) Kf (°C/m) 0.512 1.86 1.22 1.99 3.67 2.53 2.02 m. °C. 5.12 9 more group attempts remaining

Part A What is the value of A-G for the reaction MCI, 6 H₂O(s) MCL, (s) + 6 H₂O(g) - when the pressure of water vapour is 28.7 mbar? Express your answer as an integer with the appropriate units. A.G= Value μA Submit Request Answer Part B A.G' = What is the value of A,C? Express your answer with the appropriate units. μA Units Value Units ? Submit Previous Answers Request Answer Un input for part B ? X Incorrect; Try Again; 5 attempts remaining