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In 180 gram water 10g each of A,B & C ar...

In 180 gram water 10g each of A,B & C are mixed separately, then correct order of vapour pressure of these solution is:
(given molecular mass of A,B & C are 100,150 & 125 g/mole respectively)

A

`AgtBgtC`

B

`BgtCgtA`

C

`AgtCgtB`

D

`CgtBgtA`

Text Solution

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To solve the problem, we need to determine the order of vapor pressure of the solutions formed by mixing 10 g of each solute (A, B, and C) in 180 g of water. The molecular masses of A, B, and C are given as 100 g/mol, 150 g/mol, and 125 g/mol, respectively. ### Step-by-Step Solution: 1. **Calculate the number of moles of each solute:** - The number of moles of a substance can be calculated using the formula: \[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \] - For solute A: \[ n_A = \frac{10 \, \text{g}}{100 \, \text{g/mol}} = 0.1 \, \text{mol} \] - For solute B: \[ n_B = \frac{10 \, \text{g}}{150 \, \text{g/mol}} = \frac{10}{150} = 0.0667 \, \text{mol} \] - For solute C: \[ n_C = \frac{10 \, \text{g}}{125 \, \text{g/mol}} = \frac{10}{125} = 0.08 \, \text{mol} \] 2. **Determine the number of moles of solutes:** - From the calculations: - Moles of A = 0.1 mol - Moles of B = 0.0667 mol - Moles of C = 0.08 mol 3. **Rank the number of moles:** - The order of the number of moles from highest to lowest is: - A (0.1 mol) > C (0.08 mol) > B (0.0667 mol) 4. **Understand the relationship between vapor pressure and number of moles:** - The vapor pressure of a solution decreases as the number of moles of non-volatile solute increases. Therefore, the solution with the highest number of moles will have the highest vapor pressure. 5. **Determine the order of vapor pressure:** - Since A has the highest number of moles, it will have the highest vapor pressure, followed by C, and then B. - Thus, the order of vapor pressure from highest to lowest is: - A > C > B 6. **Final order of vapor pressure:** - The correct order of vapor pressure of the solutions is: - **A, C, B**
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