Question

1) Consider the following equation: Rate = k [CH₃I]² [C₁₅H₁₁N]

i) If the concentration of C₁₅H₁₁N is doubled, does the rate constant:

A) Increase

B) Decrease

C) Remain unchanged

ii) If the concentration of of CH₃I is decreased by a factor of 3, the time it takes for the reaction to finish will:

A) Increase by a factor of 3

B) Increase by a factor of 9

C) Decrease by a factor of 9

D) Remain Unchanged

iii) If the temperature increases how will the activation energy change:

A) It will increase

B) It will decrease

C) It will remain unchanged

2) During a titration of a weak acid with a strong base you add an additional small amount of base after reaching the equivalence point.

i) How does the pH of the solution change?

A) Increase

B) Decrease

C) Remain unchanged

ii) How does the K_a of the acid change?

A) Increase

B) Decrease

C) Remain unchanged

Answer 1

i.Rate = k [CH₃I]² [C₁₅H₁₁N]

rate constant does not depends on the conc of reactants. If the concentration of C₁₅H₁₁N is doubled. Rate constant remain unchange.

C) Remain unchanged >>>>>answer

ii.Rate = k [CH₃I]² [C₁₅H₁₁N]

If the concentration of of CH₃I is decreased by a factor of 3

Rate = K(1/3)^2 [C₁₅H₁₁N]

rate of reaction decreases 1/9 times.

C) Decrease by a factor of 9

iii.

Activation energy is directely proportional to temperature.

A) It will increase

2. basic nature is increases PH value is increases.

A) Increase

ii.Ka is acid dissociation constant

A) Increase