In acidic solution, the breakdown of sucrose into glucose and fructose has this rate law: rate = k[H+][sucrose].
The initial rate of sucrose breakdown is measured in a solution that is 0.01 M H+, 1.0 M sucrose, 0.1 M fructose, and 0.1 M glucose.
How does the rate change if:
(a) [Sucrose] is changed to 2.5 M?
(b) [Sucrose], [fructose], and [glucose] are all changed to 0.5 M?
(c) [H+] is changed to 0.0001 M?
(d) [Sucrose] and [H+] are both changed to 0.1 M ?

a)If concentration of [Sucrose] is changed to 2.5 M than rate will be increased by the factor of 2.5.

b)If concentration of [Sucrose] is changed to 0.5 M than rate will be increased by the factor of 0.5.

c)If concentration of   is changed to 0.0001 M than rate will be increased by the factor of 0.01.

d) If concentration when [sucrose] and both are changed to 0.1 M than rate will be increased by the factor of 1.

Explanation:

Sucrose +    fructose+ glucose

The rate law of the reaction is given as:

[sucrose]= 1.0 M

..[1]

a)

The rate of the reaction when [Sucrose] is changed to 2.5 M = R'

..[2]

[2] ÷ [1]

If concentration of [Sucrose] is changed to 2.5 M than rate will be increased by the factor of 2.5.

b)

The rate of the reaction when [Sucrose] is changed to 0.5 M = R'

..[2]

[2] ÷ [1]

If concentration of [Sucrose] is changed to 0.5 M than rate will be increased by the factor of 0.5.

c)

The rate of the reaction when is changed to 0.001 M = R'

..[2]

[2] ÷ [1]

If concentration of   is changed to 0.0001 M than rate will be increased by the factor of 0.01.

d)

The rate of the reaction when [sucrose] and both are changed to 0.1 M = R'

..[2]

[2] ÷ [1]

If concentration when [sucrose] and both are changed to 0.1 M than rate will be increased by the factor of 1.

dynamic equilibrium is the answer.