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In the reaction aA + bB --> cC, I am given the rate of appearance for C, and this is the equation relationship that would help me find the rate of disappearance of B.
What is (-1/b)(∆B/∆t) = (1/c)(∆C/∆t)?
True or false: rate laws are dependent on both reactants and products.
FALSE
This is the equation for calculating a half-life.
What is t1/2 = 0.693/k?
This species has the greatest rate of appearance in the reaction below:
2 H₂S + O₂ → 2 S + 2 H₂O
What is both S and H2O?
In a reaction, the rate law is rate = k[CO][Br2]3. The overall order of this reaction is this.
What is 4th order?
The kinetics of a gas phase reaction of the form A → Products results in a rate constant of 1.308 M⁻¹ s⁻¹. For this reaction, the initial concentration of A is 0.527 M. This is the half-life for this reaction.
What is 1.45s?
This species has the greatest rate of disappearance in the reaction below.
CH₄ + 2O₂ → CO₂ + 2H₂O
What is O2?
Given the rate law and the table, these are the values of m and n.
https://docs.google.com/document/d/1dg4d5BskN61ahf6lbWXPA36M6t2L5WjUx3Q3nu60O5U/edit?usp=sharing
What is m=O and n=1?
This is the concentration of a reactant after 19.0s if the initial concentration is 0.150M and the rate constant is 1.20x10-2 s-1.
What is 0.119M?
At a certain point in the following reaction, the rate of disappearance of NO is measured to be 0.060M/s. This is the rate of disappearance of O2 at the same moment.
2NO + O2 → 2NO2
Determine the rate law for the given reaction.
https://docs.google.com/document/d/1dg4d5BskN61ahf6lbWXPA36M6t2L5WjUx3Q3nu60O5U/edit?usp=sharing
What is rate = k[A]?
If a reaction is first order with a rate constant of 0.0450s-1, this is how much time is required for 80% of the initial quantity of reactant to be consumed.
What is 35.76s?
At a particular moment in the following reaction, the rate of disappearance of Br- is measured to be 0.125M/s. This is the rate of appearance for Br2.
5Br- + BrO3- + 6H+ → 3Br2 + 3H2O
What is 0.075M/s?
This is the rate for the first order reaction A → Products when [A] = 0.236M. (k = 0.360min-1)
What is 0.085M/min?
On a graph, this is what the slope of the line will look like for an integrated first-order reaction.
What is a straight line negatively sloping down?