chemistry, chemical kinetics
posted by student .
I keep getting these questions wrong, could someone please help.
Thanks so much.
For the following overall reaction, the rate constant is 3.4x10^-2.
A(g)+ 2B -> 2C + D
What may be the rate reaction?
The rate law for this reaction is R=k[NO][Cl2]
Mechanism for the reaction.
NO + Cl2 -> NOCl2
NOCl2 + NO -> 2NOCl
Which of the following accurately describes this reaction?
2nd order reaction
The first step is the slow step
Doubling [NO] would quadrople the rate
Cutting [Cl2] in half would decrease the rate by a factor of 2.
The molecularity of the first step is 1.
Both steps are termolecular.
I'm not sure but for this particular question I think the answer may be 2nd order reaction and cutting [Cl2]....
the reaction is 1st order with respect to NO and 1st order with respect to Cl2 which makes it 1+1 = 2 = 2nd order overall.
Cutting Cl2 in half is also true.
Doubling NO is not true.
The molecularity of the first step is not 1.
Both steps are termolecular is not true.
atleast I know the second question can be right.
calculate the ratio of rate constants for two thermal reactions that have the same arrhenius preexponential,but with activation energies that differ by 1,10, and 30 kJ/mol for T= 298K