Question

The reaction A + 2B + C → Products has a rate law of Rate = k[A]². By what factor would the reaction rate change if is tripled?

Answer 1

Same logic as a question I believe I solved before
\(R=k\left[A\right]^{2}\left[B\right]\)
The concentration of B is now tripled, so you can plug in 3B
\(R=k\left[A\right]^{2}\left[3B\right]\)
And you can simplify to find the new R. Let me know if you have any questions.