Kinetics

Which one of the following is a first order, overall reaction

• k₁= 1.000 M s^-1
• k₁= 5403.2 M^½ s^½
• k₁= 1.23 x 10^-6 M^-1 s^-1
• k₁= 10.7 s^-1

Tags

NGSS.HS-PS1-5

• A. is most exothermic
• B. is most exothermic
• C. is most exothermic
• D. is most exothermic

Tags

NGSS.HS-PS1-4

Consider the following rate law: Rate = k[A]ⁿ[B]^m
How are the exponents n and m determined?

• by using balanced chemical equation
• By using the subscripts for the formulas
• By educated guess
• By experiment 

Tags

NGSS.HS-PS1-5

What would be my the overall order of this rate law? 
Rate=[A]²[B]¹

• 0 Order
• 1st Order
• 2nd Order
• 3rd Order

Tags

NGSS.HS-PS1-5

step 1: O₃ → O₂ + O
step 2: O₃ + O → 2 O₂

The oxygen atom (O) is considered to be a(n)...

• reactant
• catalyst
• reaction intermediate
• activated complex

The reaction of (CH₃)₃CBr with hydroxide ion proceeds:
(CH₃)₃CBr(aq) + OH^-(aq) → (CH₃)₃COH(aq) + Br^-(aq)
What will the initial rate (in mol/L*s) be in Experiment 4?

• 0.003
• 0.006
• 0.009
• 0.018

Tags

NGSS.HS-PS1-5

In any first order reaction, as the reaction proceeds at constant temperature, which describes the corresponding effects on k (the rate constant) and rate?

• k remains the same; rate decreases
• k and rate both remain the same
• k remains the same; rate increases
• k decreases; rate remains the same

Tags

NGSS.HS-PS1-5

A compound has a half-life of 14 min. How much time will it take a 12 mol sample to decay to 1.5 mol?

• 14 min
• 28 min
• 42 min
• 56 min

Tags

NGSS.HS-PS1-8

• rate = k[CO]²[O₂]²
• rate = k[CO]²[O₂]
• rate = k[CO][O₂]²
• rate = k[CO][O₂]^1/2

Tags

NGSS.HS-PS1-5

• IO^-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
• I^-, because it was used as a reactant in an earlier step and reproduced in a subsequent step
• IO^-, because it was produced in an earlier step and used up in a subsequent step
• I^-, because it was produced in an earlier step and used up in a subsequent step

Tags

NGSS.HS-PS1-2