Part 1: 6.970 g of a non-volatile solute is dissolved in 230.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 60°C the vapour pressure of the solution is 147.48 torr. The vapour pressure of pure water at 60°C is 149.40 torr. Calculate the molar mass of the solute (g/mol). Part 2: Now suppose, instead, that 6.970 g of a volatile solute is dissolved in 230.0 g of water. This solute also does not react with water nor dissociate in solution. The pure solute displays, at 60°C, a vapour pressure of 14.94 torr. Again, assume an ideal solution. If, at 60°C the vapour pressure of this solution is also 147.48 torr. Calculate the molar mass of this volatile solute.
Part 1: 6.970 g of a non-volatile solute is dissolved in 230.0 g of water.
The solute does not react with water nor dissociate in solution.
Assume that the resulting solution displays ideal Raoult's law behaviour.
At 60°C the vapour pressure of the solution is 147.48 torr.
The vapour pressure of pure water at 60°C is 149.40 torr.
Calculate the molar mass of the solute (g/mol).
Part 2: Now suppose, instead, that 6.970 g of a volatile solute is dissolved in 230.0 g of water.
This solute also does not react with water nor dissociate in solution.
The pure solute displays, at 60°C, a vapour pressure of 14.94 torr.
Again, assume an ideal solution.
If, at 60°C the vapour pressure of this solution is also 147.48 torr.
Calculate the molar mass of this volatile solute.
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