1.0 L of 2.0 M acetic acid is added with 1.0 L of 3.0 M ethyl alcohol. The following reaction takes place during this process CH3COOH+C2H5OH leftharpoons CH3COOC2H5+H2O If each solution is diluted by adding 1.0 L water, then initial rate of the reaction will reduce

Question

1.0 L of 2.0 M acetic acid is added with 1.0 L of 3.0 M ethyl alcohol. The following reaction takes place during this process CH3COOH+C2H5OH leftharpoons CH3COOC2H5+H2O If each solution is diluted by adding 1.0 L water, then initial rate of the reaction will reduce (A) 0.5 times (B) 2.0 times (C) 4.0 times (D) 0.25 times

Tardigrade Admin · Accepted Answer

CH3COOH+C2H5OH→ CH3COOC2H5+H2O This is a second order reaction. Hence, initial rate of the reaction will reduced by (1/2)2 ie, 0.25 times.

Q. 1.0 L of 2.0 M acetic acid is added with 1.0 L of 3.0 M ethyl alcohol. The following reaction takes place during this process
$C H_{3} COO H + C_{2} H_{5} O H$ $⇌ C H_{3} COO C_{2} H_{5} + H_{2} O$
If each solution is diluted by adding 1.0 L water, then initial rate of the reaction will reduce

0.5 times

2.0 times

4.0 times

0.25 times

$C H_{3} COO H + C_{2} H_{5} O H \to C H_{3} COO C_{2} H_{5} + H_{2} O$ This is a second order reaction. Hence, initial rate of the reaction will reduced by (1/2)2 ie, 0.25 times.

Q. 1.0 L of 2.0 M acetic acid is added with 1.0 L of 3.0 M ethyl alcohol. The following reaction takes place during this process CH3​COOH+C2​H5​OH ⇌CH3​COOC2​H5​+H2​O If each solution is diluted by adding 1.0 L water, then initial rate of the reaction will reduce