Question

1. You made wintergreen in Lab 1 by reacting salicylic acid (C 7H,O3) with methanol (CH3OH). If you react salicylic acid with acetic acid (C2H402). you can make aspirin The rate law for this reaction is: rate k [C H6o3 IC2H421 The salicylic acid and acetic acid reaction is slow. Sulfuric acid, H2SO4, is used as a catalyst in this reaction. The rate law for this reaction with the H2SO4 catalyst is: rate k [C 2H,02l [H2SO, a. If the reaction is run at 25oC instead of 70oC, the rate constant increases O decreases O stays the same b. What equation or formula supports your answer? Write the equation. Do not give its name Your answer c. Using a catalyst increases the: Check the boxes that apply rate law rate constant activation energy temperature reaction mechanism

Answer 1

A) The temperature is decreases from 70C to 25C, the rate constant is also decreases.

rate constant is decreases when the temperature is decreases.

The answer is B

B)

Temperature effect on rate constant explains with the help of Arrhenious equation.

lnK= Ae^-Ea/RT

K= rate constant

A= Arrhenious factor

Ea = activation energy

R= gas constant

T= temperature

C) when the catalyst is added to the reaction mixture,the reaction mechanism increases.

The reaction mechanism increases, the more number of reactant species undergo chemical reaction by decreasing the activation energy of the system.

The answer is reaction mechanism.