My question is about number 5. It uses information from number 4. A liquid-phase

Question

My question is about number 5. It uses information from number 4.

A liquid-phase mixture of 450 mL of acetic acid. 300 mL of ethanol. 2.00 mL of water, and 2.00 mL ethyl acetate are mixed together at 298 K. where the following reaction will occur: CH_3COOCH_2 CH_3 + H_2O CH_3COOH + CH_3CH_2 OH, k_c = 3440 . Will the reaction occur from left-to-right or right-to-left (as written)? Please support your answer. For the reaction and conditions described for Problem 4, show that 0.0507 moles of each reactant are converted into each product (i.e., 0.0507 mol of water and 0.0507 mol of ethyl acetate are converted into 0.0507 mol of acetic acid and 0.0507 mol of ethanol; or. vice versa).

Explanation / Answer

Solution :-

Kc = 3440

Kc is very high therefore the forward reaction will take place that means the 0.0507 mol ethyl acetate and 0.0507 mol H2O will convert to the 0.0507 mol acetic acid and 0.0507 mol ethanol

Reaction equation is as follows

CH3COOCH2CH3 + H2O ------- > CH3COOH + CH3CH2OH

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