Hello please answer this question attached below: ### Freezing Point Depression DataThe following data was collected during the preparation of a solution:| Mass unknown solute (g) | Mass solvent (g) | \( T_f \) (solvent) (°C) | \( T_f \) (solution) (°C) | \( k_f \) (°C·kg/mol) ||-------------------------|------------------|------------------------|------------------------|--------------------------|| 0.117 | 5.28 | 6.30 | 2.62 | 6.50 |#### Tasks:a. **Calculate the \(\Delta T_f\) for the solution using the equation given above.**b. **The solute is a nonelectrolyte. Using the equation (2) above, find the molality of the solution.**c. **Calculate the moles of the unknown solute.**d. **Calculate the molar mass of the unknown solute.**#### Explanation:- **\(\Delta T_f\)** represents the change in freezing point of the solution.- **Molality** is a measure of the number of moles of solute per kilogram of solvent.- **Nonelectrolyte** implies that the solute does not dissociate into ions in the solution.- **Moles of solute** can be calculated via the molality and mass data.- **Molar mass** is the mass of one mole of a substance.### Example Calculations:1. **Calculate \(\Delta T_f\)**: \(\Delta T_f = T_f(\text{solvent}) - T_f(\text{solution}) = 6.30^\circ \text{C} - 2.62^\circ \text{C} = 3.68^\circ \text{C}\)2. **Find the molality of the solution**: Using the formula: \[ \Delta T_f = k_f \cdot m \] where \( \Delta T_f \) is the freezing point depression, \( k_f \) is the freezing point depression constant, and \( m \) is the molality. \[ 3.68^\circ \text{C} = 6.50^\circ \text{C·kg/mol} \cdot m \] Solving

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2. The following data was collected as a solution was prepared. Mass unknown solute (g) Mass solvent (g) Tf(solvent) (°C) Tf(solution) (°C) kf(°C-kg/mol) 0.117 6.30 2.62 6.50 5.28 a. Calculate the AT, for the solution using equation (1) above. b. The solute is a nonelectrolyte. Using equation (2) above, find the molality of the solution. c. Calculate the moles of the unknown solute. d. Calculate the molar mass of the unknown solute.