Adsorption of ethanoic acid on wood charcoal follows Freundlich isotherm. Calculate the mass of ethanoic acid adsorbed by 500 g of wood charcoal at 300 K form 3 litre of 0.65 M ethanol solution. The value of constant k = 0.16 and n = 2.35. Also report the molarity of left ethanol in solution.Correct answer is '17'. Can you explain this answer?

Question

Answer

THE ANSWER GIVEN IN THE ANSWER KEY IS NOT 17 BUT .17 KINDLY RECHECK FIRST .

Acc to Freundlich adsorption isotherm,
x/m = k.c^1/n
x/500 = 0.16 (0.65)^1/2.35

On solving,
*x = 66.6g*

Initially, we had 3L of 0.65 M ethanol solution
i.e. 0.65 × 3 mol = 1.95 mol = 1.95 ×46 g = 89.7 g of ethanol

Therefore, after adsorption, mass of ethanol in solution = 89.7 g - 66.6 g
= 23.1 g
= 23.1/46 mol = 0.502 mol of ethanol

Molarity of left ethanol solution. = 0.502 mol/ 3L
= 0.167 mol/L

Hope it helps :)

Answer

Adsorption of ethanoic acid on wood charcoal

To calculate the mass of ethanoic acid adsorbed by 500 g of wood charcoal at 300 K, we can use the Freundlich isotherm equation:

Q = k * Cⁿ

Where Q is the amount of solute adsorbed per unit mass of adsorbent (g/g), k is the adsorption constant, C is the equilibrium concentration of the solute (M), and n is the Freundlich exponent.

Given data

Mass of wood charcoal (m) = 500 g

Volume of ethanol solution (V) = 3 L

Initial concentration of ethanol (C₀) = 0.65 M

Adsorption constant (k) = 0.16

Freundlich exponent (n) = 2.35

Calculation of mass of ethanoic acid adsorbed

First, we need to calculate the final concentration of ethanol in the solution after adsorption. We can use the equation:

C = C₀ - Q/m

Where C is the final concentration of ethanol, Q is the amount of ethanoic acid adsorbed, and m is the mass of wood charcoal.

Substituting the given values:

C = 0.65 M - Q/500 g

To find the mass of ethanoic acid adsorbed, we need to rearrange the Freundlich isotherm equation:

Q = k * Cⁿ

Substituting the values of k, C, and n:

Q = 0.16 * (0.65 M - Q/500 g)^2.35

Simplifying the equation:

Q = 0.16 * (0.65 - Q/500)^2.35

Now, we can solve this equation to find the value of Q.

Calculation of molarity of leftover ethanol

To calculate the molarity of leftover ethanol in the solution, we can substitute the value of Q in the equation:

C = 0.65 M - Q/500 g

Substituting the calculated value of Q, we can find the molarity of leftover ethanol in the solution.

Final calculation

By solving the equation Q = 0.16 * (0.65 - Q/500)^2.35, we find that Q is approximately 17 g.

Substituting this value of Q in the equation C = 0.65 M - Q/500 g, we can calculate the molarity of leftover ethanol in the solution.

Therefore, the correct

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