the rate constant of a chemical reaction increased from .100s-1 to 2.90s-1 upon
ID: 883362 • Letter: T
Question
the rate constant of a chemical reaction increased from .100s-1 to 2.90s-1 upon raising the temperature from 25 C to 45C. calculate the value of (1/t2-1/t1) where t1 is the initial temperature and t2 is the finial temperature K-1?Also, calculate the bailey on In where k1 and k2 corresponds to the rate constant at the initial and the final temperature as above (k1/k2) In=?
Also, what is the activation energy of the reaction in kJ/mol Ea=?
the rate constant of a chemical reaction increased from .100s-1 to 2.90s-1 upon raising the temperature from 25 C to 45C. calculate the value of (1/t2-1/t1) where t1 is the initial temperature and t2 is the finial temperature K-1?
Also, calculate the bailey on In where k1 and k2 corresponds to the rate constant at the initial and the final temperature as above (k1/k2) In=?
Also, what is the activation energy of the reaction in kJ/mol Ea=?
the rate constant of a chemical reaction increased from .100s-1 to 2.90s-1 upon raising the temperature from 25 C to 45C. calculate the value of (1/t2-1/t1) where t1 is the initial temperature and t2 is the finial temperature K-1?
Also, calculate the bailey on In where k1 and k2 corresponds to the rate constant at the initial and the final temperature as above (k1/k2) In=?
Also, what is the activation energy of the reaction in kJ/mol Ea=?
Explanation / Answer
1)(1/T1-1/T2)=(1/298-1/318)=(0.0033-0.0031)k-1=0.0002 K-1
2)ln k1/k2= ln 100/2.9=34.48
3)Using Arrhenius equation, ln k2/k1=Ea/kb(1/T1-1/T2) where Ea=activation energy and R=gas constant
ln 2.90/100=Ea/ 8.314J K-1 mol-1 *(1/298-1/318)
ln 0.029=Ea/8.314J K-1 mol-1(0.0033-0.0031)k-1
-3.54=Ea *2.40* 10^ -5 J mol-1
Ea=-1.475 *10^ 5 J mol-1
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