Question

2a

Calculate the freezing point of a solution that is made from 39.9 g of a nonelectrolyte (ℳ = 142.4701 g/mol) dissolved in 186.3 g of solvent. The solvent freezes at 1.24 °C and its K_f value is 2.09 °C/m.

Report your answer to TWO places past the decimal.

2b

The solubility of carbon dioxide gas at 37.3 °C and a carbon dioxide pressure of 554 mmHg is 4.04 × 10⁻³ g/L. What is the Henry's Law constant in mol⋅L⁻¹⋅atm⁻¹?

Report your answer to THREE significant figures. You may (but are not required to) enter your answer in scientific notation; for example, if your answer is 2.44 × 10⁻², you would enter 2.44E-2. The E must be uppercase.

2c.

When a solution is made from 31 g of an unknown nonelectrolyte dissolved in 137.4 g of solvent, the solution boils at 80.56 °C. The boiling point of the pure solvent and its K_b are 73.75 °C and 4.17 °C/m, respectively. Calculate the molar mass of the unknown electrolyte in g/mol.

Report your answer to TWO places past the decimal.

2d

Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.4 gdissolved in 211.9 mL of water at 42.21 °C has an osmotic pressure of 44 mmHg.

R = 0.082058 L⋅atm⋅mol⁻¹⋅K⁻¹. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures.

2e

What is the solubility (in mol/L) of nitrogen gas at a pressure of 340 mmHg? The Henry's Law constant, K_H is 6.54 × 10⁻⁴ mol⋅L⁻¹⋅atm⁻¹.

Report your answer to THREE significant figures. You may (but are not required to) enter your answer in scientific notation; for example, if your answer is 2.44 × 10⁻², you would enter 2.44E-2. The E must be uppercase.

thank you!!

Answer 1