The reaction A+B⟶C+Drate=𝑘[A][B]2 has an initial rate of 0.0940 M/s. What will the initial rate be if [A] is halved and
Posted: Mon Jul 11, 2022 1:53 pm
The reaction
A+B⟶C+Drate=𝑘[A]2
has an initial rate of 0.0940 M/s.
What will the initial rate be if [A] is halved and istripled?
initial rate: ? M/s
What will the initial rate be if [A] is tripled and ishalved?
initial rate: ? M/s
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The rate constant for this first‑order reaction is 0.310 s−1 at400 ∘C.
A⟶products
How long, in seconds, would it take for the concentration of Ato decrease from 0.870 M to 0.250 M?
𝑡= ? s
----
After 49.0 min, 27.0% of a compound has decomposed. What is thehalf‑life of this reaction assuming first‑order kinetics?
𝑡1/2= ? min
----
The rate constant for this second‑order reaction is 0.410M−1⋅s−1 at 300 ∘C.
A⟶products
How long, in seconds, would it take for the concentration of Ato decrease from 0.830 M to 0.220 M?
𝑡= ? s
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Calculate the rate constant, 𝑘, for a reaction at 64.0 °C thathas an activation energy of 85.3 kJ/mol and a frequency factor of1.56×1011 s−1.
𝑘= ? s−1
A+B⟶C+Drate=𝑘[A]2
has an initial rate of 0.0940 M/s.
What will the initial rate be if [A] is halved and istripled?
initial rate: ? M/s
What will the initial rate be if [A] is tripled and ishalved?
initial rate: ? M/s
------
The rate constant for this first‑order reaction is 0.310 s−1 at400 ∘C.
A⟶products
How long, in seconds, would it take for the concentration of Ato decrease from 0.870 M to 0.250 M?
𝑡= ? s
----
After 49.0 min, 27.0% of a compound has decomposed. What is thehalf‑life of this reaction assuming first‑order kinetics?
𝑡1/2= ? min
----
The rate constant for this second‑order reaction is 0.410M−1⋅s−1 at 300 ∘C.
A⟶products
How long, in seconds, would it take for the concentration of Ato decrease from 0.830 M to 0.220 M?
𝑡= ? s
---
Calculate the rate constant, 𝑘, for a reaction at 64.0 °C thathas an activation energy of 85.3 kJ/mol and a frequency factor of1.56×1011 s−1.
𝑘= ? s−1