Please help What is the freezing point of a solution containing 2.80 grams benze
ID: 783053 • Letter: P
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What is the freezing point of a solution containing 2.80 grams benzene (molar mass =78.11 g/mol ) dissolved in 43.0 grams par dichlorobenzene (molar mass = 147.0 g/mol)? The freezing point of pure para is 53.0 degree c and the freezing point depression constant, Kfp, is -7.10 degree C/m. 47.7 degree c 47.1 degree c 58.9 degree c 52.6 degree c 58.9 degree c What is the boiling point of a solution containing 0.852 g napthalence (c10H8 mallar mass = 128.2 g/mol) dissolved in 14.0 g benzene? The boiling point of pure benzene is 80.10 degree c and the be loving constant Kbp, is 2.53 degree c/m. 78.70 degree c 80.25 degree c 81.30 degree c 82.50 degree c 85.43 degree c The osmotic pressure of blood is 7.65 atm at 37 degree C. What mass of glucose (C6H1206, molar mass - 180.2 g/mol) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (R = 0.08206 L-atm/mol-K) 0.676 g 0.698 g 5.67 g 122 g 1.02 times 103 g You dissolve 92.0 grams of CH3CH2OH (molar mass = 46.07 g/mol), ethanol, in 270. g of water (molar mass = 18.02 g/mol). What is the modality of ethanol in the solution? 341 m 170 m 0.341 m 7.40 m none of the above Given the heat of formation data below: delta H degree [LiOH(s)] = - 484.93 kj/mol, and delta ,H degree [LiOH(aq)] = - 508.48 kJ/mol. Calculate delta solution H for the following process: LiOH(s) rightarrow LiOH(aq) +23.55 kJ/mol +993.41 kJ/mol -23.55 kJ/mol -993.41 kJ/mole. none of the aboveExplanation / Answer
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