rate law
The elementary rate law for the reaction:
CH4 + 2O2 --> CO2 + 2H2O
What is rate=k[CH4][O2]2?
Present at the beginning of the reaction.
What is a reactant?
The order for H2 in the reaction
H2(g) + Cl2(g) --> 2 HCl(g)
with the following experimental data:
Ex [ H2] [Cl2] RoF of HCl
1 0.00100 0.000500 1.82×10-12
2 0.00200 0.000500 3.64×10-12
3 0.00200 0.000250 1.82×10-12
What is n = 1?
The t1/2 when n=1 and k=1.50x10-6 min-1?
What is 4.62x105 min?
The overall equation for the gas-phase decomposition of nitrous oxide with the following two-step mechanism.
Step 1: N2O --> N2 + O
Step 2: O + N2O --> N2 + O2
What is 2N2O --> 2N2 + O2?
Rate law is written as: rate equals rate constant times each reactant to their coefficients as exponents from this step in a reaction mechanism.
What is the slow step OR rate determining step?
Present at the end of the reaction.
What is a product?
The order for Cl2 in the reaction
H2(g) + Cl2(g) --> 2 HCl(g)
with the following experimental data:
Ex [ H2] [Cl2] RoF of HCl
1 0.00100 0.000500 1.82×10-12
2 0.00200 0.000500 3.64×10-12
3 0.00200 0.000250 1.82×10-12
What is n=1
The rate constant when n=1 and t1/2=3.84x10-7 s?
What is 1.80x106 s-1?
The intermediate species in the gas-phase decomposition of nitrous oxide with the following two-step mechanism.
Step 1: N2O --> N2 + O
Step 2: O + N2O --> N2 + O2
What is O?
The rate law for the reaction
Na2CO3 + CO2 + H2O --> 2NaHCO3
When n=0 for CO2; n=1 for Na2CO3; and n=2 for H2O
What is rate=k[Na2CO3][H2O]2?
Made in the reaction, but now present at the end of the reaction.
What is an intermediate?
The overall order for the reaction
H2(g) + Cl2(g) --> 2 HCl(g)
with the following experimental data:
Ex [ H2] [Cl2] RoF of HCl
1 0.00100 0.000500 1.82×10-12
2 0.00200 0.000500 3.64×10-12
3 0.00200 0.000250 1.82×10-12
What is n=2
The value of the rate constant for a second order reaction if the reactant
concentration drops from 0.657 M to 0.0981 M in 17.0 s.
What is 0.510 M-1s-1?
The overall reaction for the following steps.
STEP 1: NO2(g) + NO2(g) <-> N2O4(g)
FAST EQUILIBRIUM Exothermic
STEP 2: N2O4(g) --> 2NO(g) + O2(g)
SLOW Endothermic
What is
NO2(g) + NO2(g) --> 2NO(g) + O2(g)
The value of k in the rate law: rate=k[NO][O2]2
when [NO]=0.0526; [O2]=0.604; rate=1.56x10-6mol*L*s-1
what is k=8.13x10-5 s-1?
Not a part of the reaction. Decreases activation energy.
What is a catalyst?
The order when concentration changes by 5 and initial rate changes by 25.
What is n=2?
The [H2O2] after 10 minutes if [H2O2]0 is 0.200 M.
The decomposition of H2O2 to water and oxygen follows first order kinetics with a rate constant of 0.0410 min-1.
What is [H2O2]=0.132M?
The rate determining step for the following reaction mechanism.
STEP 1: NO2(g) + NO2(g) <-> N2O4(g)
FAST EQUILIBRIUM Exothermic
STEP 2: N2O4(g) --> 2NO(g) + O2(g)
SLOW Endothermic
What is STEP 2:
N2O4(g) --> 2NO(g) + O2(g)
The initial concentration of NO in the reaction when rate = k[NO]2
rate=1.50x10-3
k=202.66
What is 2.72x10-3 M = [NO]?
governs the rate of the entire reaction.
What is the rate determining step?
The order when concentration changes by 35.678 and initial rate stays equal.
What is n=0?
The first t1/2 when n=0 and the reactant
concentration drops from 0.942 M to 0.351 M in 54.5 s.
What is 43.4 s?
The slow step for the gas-phase decomposition of nitrous oxide with the following two-step mechanism when rate=k[N2O].
Step 1: N2O --> N2 + O
Step 2: O + N2O --> N2 + O2
What is Step 1: N2O --> N2 + O