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26 Nov 2019

The rate constant of a chemical reactionincreased from 0.100 s%u22121 to 3.20s%u22121 upon raising the temperaturefrom 25.0 %u2218C to55.0%u2218C.
Part A
Calculate the value of (1T2%u22121T1) where T1 is the initial temperature andT2 is the final temperature.
Express your answernumerically.


Part B
Calculate the value of ln(k2k1) where k1 and k2 correspond to the rate constantsat the initial and the final temperatures as defined in partA.
Express your answernumerically

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Sixta Kovacek
Sixta KovacekLv2
24 Jul 2019

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Related questions

The rate constant of a chemical reaction increased from 0.100s?1 to 3.20s?1 upon raising the temperature from 25.0 ?C to 49.0?C.

Part A

Calculate the value of (1T2?1T1) whereT1 is the initial temperature and T2 is the finaltemperature.

Express your answer numerically.

Part B

Calculate the value of ln(k1k2) wherek1 and k2 correspond to the rate constants at theinitial and the final temperatures as defined in part A.

Express your answer numerically.

Part C

What is the activation energy of the reaction?

Express your answer numerically in kilojoules per mole.

The rate constant of a chemical reaction increased from 0.100 s−1 to 3.20 s−1 upon raising the temperature from 25.0 ∘C to 39.0 ∘C

a) Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature.

b) Calculate the value of ln(k1/k2) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.

c) What is the activation energy of the reaction?

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The rate constant of a chemical reaction increased from 0.100 s−1 to 3.00 s−1 upon raising the temperature from 25.0 ∘C to 35.0 ∘C .

Part A

Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature.

Express your answer numerically.

Part B

Calculate the value of ln(k1k2) where k1 and k2 correspond to the rate constants at the initial and the final temperatures as defined in part A.

Express your answer numerically.

Part C

What is the activation energy of the reaction?

Express your answer numerically in kilojoules per mole.

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