Is this a Brønsted–Lowry acid–base reaction?

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The discussion centers on the reaction between sulfuric acid and potassium hydroxide, which produces salt and water, indicating it is an acid-base reaction. The main inquiry is whether this reaction qualifies as a Brønsted–Lowry acid-base reaction. To determine this, participants are encouraged to review the definitions of Brønsted–Lowry acids and bases and compare them with the characteristics of sulfuric acid and potassium hydroxide. The distinction between Brønsted–Lowry and other acid-base theories, such as Arrhenius and Lewis, is also highlighted as a critical point for understanding. Ultimately, clarity on these definitions will help confirm the classification of the reaction.
Saracen Rue
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Homework Statement


A solution of sulfuric acid is added to a solution of potassium hydroxide. Write a balanced equation for this and identify whether or not this is a Brønsted–Lowry acid–base reaction.

Homework Equations


N/A

The Attempt at a Solution


I understand how to write the equation just fine, and I've identified the type of reaction as being an acid + base = salt + water. However, I am unsure of if this is the same as a Brønsted–Lowry acid–base reaction. I am thinking they are different, but I don't really have any justification for this, so any help is greatly appreciated.
 
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A good starting place would be to review the definition of Bronsted-Lowry acids and bases and see if sulfuric acid and potassium hydroxide fit those definitions.
 
Also, see the main point where Bronsted Lowry becomes unique...That is, what makes it different from Arrhenius, or Lewis acid base pairs.
Good luck!
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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