<p>I'm having trouble figuring this question out. The teacher did not explain how to do these specific kinds of questions so I was wondering how I can solve it.</p>
<p>Methyl acetate, CH3COOCH3, reacts in basic solution to give acetate ion, CH3COO-, and methanol, CH3OH.
CH3COOCH3 (aq) + OH- (aq) → CH3COO- (aq) + CH3OH (aq)
The overall order of the reaction was determined by starting with methyl acetate and hydroxide ion at the same concentrations, so [CH3COOCH3] = [OH ‾ ] = x. Then: Rate = k [CH3COOCH3]m [OH ‾ ]n = kxm + n. Determine the overall order and the value of the rate constant by plotting the following data assuming first- and then second-order kinetics.
Time (min) <strong><a href="mol/L">CH3COOCH3</a>
0.00 </strong><strong><em>0.01000
3.00 </em></strong><strong><em>0.00740
4.00 _</em></strong><strong><em>0.00683
5.00 _</em></strong><strong><em>0.00634
10.00</em></strong><strong><em>0.00463
20.00</em></strong>_<strong><em>0.00304
30.00</em></strong>__0.00224</p>
<p>I think the overall order is 2 but I'm not sure.
What is the rate constant in L/(mol·s) ?</p>