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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(d) [Sucrose] and [H⁺] are both changed to 0.1 M?

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The rate change if(d) [Sucrose] and [H⁺] are both changed to 0.1 M will increase by a factor of 1.

What is an acidic solution?

An acidic solution is a solution whose pH is lesser than 7. A pH less than 7 is the acidic solution. The breakdown of glucose into fructose.

Sucrose + H+ =  fructose + glucose

The rate law of reaction is R = k [H+] [sucorse]

H+ = 0.01 M

[sucrose] = 1.0 M

R = k [0.01M] [1.0 M]

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

R' = [0.1M] [0.1M]

2 / 1

[tex]\dfrac{R'}{R} = \dfrac{ [0.1M] [0.1M]}{ k [0.1M] [0.1M]}[/tex]

R' = 1 x R

Thus, the rate change will be increased by 1.

To learn more about the acidic solutions, refer to the below link:

https://brainly.com/question/13655896

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