chemistry
1)
The activation energy of a certain reaction is 35.3 kJ/mol. At 20 degrees C, the rate constant is 0.0130 s^1. At what temperature would this reaction go twice as fast?
Answer in units of degrees Celsius.
i think the answer is around 34, but i keep in getting it screwed up.
2)
Consider the following multistep reaction:
C + D <> CD (fast)
CD + D > CD2 (slow)
CD2 + D > CD3 (fast)
C + 3D > CD3 (overall)
determine the rate law for the overall reaction
Answer should be in k[A][B]^2 format
I know the overall reaction has much to do with the slow reaction, but i don't get how to incorporate that into its proper format based on its order
3)
The reactant concentration in a zeroorder reaction was 0.100 M after 125 s and 1.50×10−2 M after 385 s. What is the rate constant for this reaction?
What was the initial reactant concentration for the reaction?
I found the rate constant to be 3.27 x 10^4 M/s, but im having trouble finding initial reactant concentration...
an equation that mite help..
[A]=  kt + [A]0
[A]0 is the initial reactant rate i beleieve.. i thinks...

1)
The activation energy of a certain reaction is 35.3 kJ/mol. At 20 degrees C, the rate constant is 0.0130 s^1. At what temperature would this reaction go twice as fast?
Answer in units of degrees Celsius.
i think the answer is around 34, but i keep in getting it screwed up.
How are you solving it? Post your work and I'll try to find the error. You should be using the Arrhenius equation.
Also, make sure activation energy is J/mol. Also make sure you are using temperature in Kelvin.
posted by DrBob222

3)
The reactant concentration in a zeroorder reaction was 0.100 M after 125 s and 1.50×10−2 M after 385 s. What is the rate constant for this reaction?
What was the initial reactant concentration for the reaction?
I found the rate constant to be 3.27 x 10^4 M/s, but im having trouble finding initial reactant concentration...
an equation that mite help..
[A]=  kt + [A]0
[A]0 is the initial reactant rate i beleieve.. i thinks...
Can't you simply take the initial equation you had, which is,
[A] = [A]_{o}  kt (that's how you found k is it not?), then
substitute A = 0.1 and substitute your value of k, and 125 for t, then solve for [A]_{o}? You could also use 1.5 x 10^2 for (A) and 385 for t and your value of k and get the same value although I didn't try it. Check my thinking. I found about 0.14 M or so using the first suggetion above.posted by DrBob222

whatahshahahaahahahayyyhhsshhshshhshshshshshsshshshshsshshshshshshshshhshshhshsshshshshhhhhhhhhhhhhhhhhhssssssssssssssssshhhhhhhhhhhhhhhhssssssssssssssssshhhhhhhhhhhhhhhhssshhhhhhhhhhhhhhhhhssssssssssssshhhhhhhhhhhhhhsssssssssssssssssssshhhhhhhhhhhhhhh
posted by Anonymous

you suck
posted by i dont like your answers
Respond to this Question
Similar Questions

Arrhenius Question
The activation energy of a certain reaction is 32.9 kJ/mol At 25 degrees C the rate constant is 0.0160 units s1 units. At what temperature in degrees Celsius would this reaction go twice as fast? Given that the initial rate 
Arrhenius Reaction
The activation energy of a certain reaction is 32.9 kJ/mol At 25 degrees C the rate constant is 0.0160 units s1 units. At what temperature in degrees Celsius would this reaction go twice as fast? Given that the initial rate 
Temperature and Rate
Q: The activation energy of a certain reaction is 32.9 kJ/mol At 25 degrees C the rate constant is 0.0160 units s1 units. At what temperature in degrees Celsius would this reaction go twice as fast? My work: ln(0.0160/0.032) = 
Chemistry
The activation energy of a certain reaction is 34.9kJ/mol . At 23 ∘C , the rate constant is 0.0190s−1. At what temperature in degrees Celsius would this reaction go twice as fast? 
chem
The activation energy of a certain reaction is 30.3 kJ/mol. At 20 C, the rate constant is 0.0130 s^{1}. At what temperature would this reaction go twice as fast? Can't you use Arrhenius' equation for this. Look it up. You have 
chemistry
I have two questions that I really don't understand. The first one is: A reaction proceeds with delta H=10kJ/mol. The energy of activation of the uncatalyzed reaction is 150kJ/mol, whereas it is 100kJ/mol for the uncatalyzed 
Corrected Temperature Problem
Q: The activation energy of a certain reaction is 32.9 kJ/mol At 25 degrees C the rate constant is 0.0160 units s1 units. At what temperature in degrees Celsius would this reaction go twice as fast? My work: ln(0.0160/0.032) = 
Chemistry 104
A reaction rate doubles when the temperature increases from 0 degrees Celsius to 10 degrees Celsius, maintaining everything else equal. What is the activation energy for this reaction? (R = 8.314 J/mol K) 
Chemistry 104
A reaction rate doubles when the temperature increases from 0 degrees Celsius to 10 degrees Celsius, maintaining everything else equal. What is the activation energy for this reaction? (R = 8.314 J/mol K) 
help help help chemistry
why will no one answer this question? For a one step reaction, the activation energy for the forward reaction is 40.0 kJ/mol and the enthalpy of reaction is 20.0 kJ /mol. Which statement below is true? a. The activation energy of