Chemistry

Chemistry, 09.07.2019 16:30, destineedhuber8301

The activation energy of a reaction is 56.9 kj/mol and the frequency factor is 1.5×1011/s. part a calculate the rate constant of the reaction at 25 ∘c.

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Chemistry, 22.07.2019 17:30, tadams9922

The arrhenius equation shows the relationship between the rate constant k and the temperature t in kelvins and is typically written as k=ae−ea/rt where r is the gas constant (8.314 j/mol⋅k), a is a constant called the frequency factor, and ea is the activation energy for the reaction. however, a more practical form of this equation is lnk2k1=ear(1t1−1t2) which is mathmatically equivalent to lnk1k2=ear(1t2−1t1) where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (t1 and t2).part athe activation energy of a certain reaction is 44.8 kj/mol . at 28 ∘c , the rate constant is 0.0180s−1. at what temperature in degrees celsius would this reaction go twice as fast? express your answer with the appropriate units.part b given that the initial rate constant is 0.0180s−1 at an initial temperature of 28 ∘c , what would the rate constant be at a temperature of 190 ∘c for the same reaction described in part a? express your answer with the appropriate units.

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Physics, 18.09.2019 01:30, thevampsrock3

He arrhenius equation shows the relationship between the rate constant k and the temperature t in kelvins and is typically written as k=ae−ea/rt where r is the gas constant (8.314 j/mol⋅k), a is a constant called the frequency factor, and ea is the activation energy for the reaction. however, a more practical form of this equation is lnk2k1=ear(1t1−1t2) which is mathematically equivalent to lnk1k2=ear(1t2−1t1) where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (t1 and t2). part a the activation energy of a certain reaction is 39.4 kj/mol . at 28 ∘c , the rate constant is 0.0140s−1 . at what temperature in degrees celsius would this reaction go twice as fast

Answers: 2

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Chemistry, 08.10.2019 03:20, jonlandis6

The arrhenius equation shows the relationship between the rate constant k and the temperature t in kelvins and is typically written as k=ae−ea/rt where r is the gas constant (8.314 j/mol⋅k), a is a constant called the frequency factor, and ea is the activation energy for the reaction. however, a more practical form of this equation is lnk2k1=ear(1t1−1t2) which is mathematically equivalent to lnk1k2=ear(1t2−1t1) where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (t1 and t2). part a the activation energy of a certain reaction is 45.6 kj/mol . at 30 ∘c , the rate constant is 0.0160s−1 . at what temperature in degrees celsius would this reaction go twice as fast

Answers: 2

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Physics, 08.10.2019 18:00, mahogany139

He arrhenius equation shows the relationship between the rate constant k and the temperature t in kelvins and is typically written as k=ae−ea/rt where r is the gas constant (8.314 j/mol⋅k), a is a constant called the frequency factor, and ea is the activation energy for the reaction. however, a more practical form of this equation is lnk2k1=ear(1t1−1t2) which is mathematically equivalent to lnk1k2=ear(1t2−1t1) where k1 and k2 are the rate constants for a single reaction at two different absolute temperatures (t1 and t2). part a the activation energy of a certain reaction is 39.4 kj/mol . at 28 ∘c , the rate constant is 0.0140s−1 . at what temperature in degrees celsius would this reaction go twice as fast

Answers: 1

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The activation energy of a reaction is 56.9 kj/mol and the frequency factor is 1.5×1011/s. part a ca...

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