Question

The hydrolysis of hydrogencarbonate ions in water at high pH is shown in the following equation (equation 2): HCO3- + OH- ? CO32- + H2O Equation 2 follows the rate law: Rate = k[HCO3-], where k = 0.01 s-1 at 25 °C a) State what is the overall order of the reaction? b) What is the half-life of HCO3- if the initial concentration of HCO3-, [HCO3-]0 = 0.001 mol dm-3? c) What is the rate constant of the above reaction at 350 K if the activation energy is 10.0 kJ mol-1?

          The hydrolysis of hydrogencarbonate ions in water at high pH is shown in the
following equation (equation 2):

HCO3- + OH- ? CO32- + H2O
Equation 2

follows the rate law: Rate = k[HCO3-], where k = 0.01 s-1 at 25 °C

a) State what is the overall order of the reaction?

b) What is the half-life of HCO3- if the initial concentration of HCO3-, [HCO3-]0 =
0.001 mol dm-3?

c) What is the rate constant of the above reaction at 350 K if the activation energy
is 10.0 kJ mol-1?

The hydrolysis of hydrogencarbonate ions in water at high pH is shown in the
following equation (equation 2):

HCO3- + OH- ? CO32- + H2O
Equation 2

follows the rate law: Rate = k[HCO3-], where k = 0.01 s-1 at 25 °C

a) State what is the overall order of the reaction?

b) What is the half-life of HCO3- if the initial concentration of HCO3-, [HCO3-]0 =
0.001 mol dm-3?

c) What is the rate constant of the above reaction at 350 K if the activation energy
is 10.0 kJ mol-1?

Added by Teresa S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Shyam P

04/05/2022

Step 1

In this case, the rate law is given as Rate = k[HCO3-], where the power of [HCO3-] is 1. Therefore, the overall order of the reaction is 1. Show more…

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The hydrolysis of hydrogencarbonate ions in water at high pH is shown in the following equation (equation 2): HCO3- + OH- → CO32- + H2O Equation 2 follows the rate law: Rate = k[HCO3-], where k = 0.01 s-1 at 25 °C a) State what is the overall order of the reaction? b) What is the half-life of HCO3- if the initial concentration of HCO3-, [HCO3-]0 = 0.001 mol dm-3? c) What is the rate constant of the above reaction at 350 K if the activation energy is 10.0 kJ mol-1?