Suppose a chemical reaction is first order and has a half-life of 2.5 hr at 100...

Suppose a chemical reaction is first order and has a half-life of 2.5 hr at 100 ºC. Which of the following statements is false regarding this reaction if the temperature is changed?

Question 5 options:

A)	The half-life at 125 ºC is 1.8 hr.

B)	The half-life at 275 ºC is 3.5 hr.

C)	The half-life at 75 ºC is 4.7 hr.

D)	Not enough information has been provided in order to make a conclusion.

Solutions

Expert Solution

Sol.

For a first order reaction ,

Rate constant = k = 0.693 / t1/2 ( equation 1 )

where t1/2 is half - life

Also , Arrhenius equation is :

ln ( k2 / k1 ) = ( Ea / R ) × ( T2 - T1 ) / ( T2 × T1 )

( equation 2 )

where k2 and k1 are rate constants at temperatures T2 and T1 respectively

Ea is activation energy and R is gas constant

So , with the help of equations 1 and 2 , we can calculate half - lifes at different temperatures

But the value of activation energy , Ea is not provided in the question . So , it is impossible to calculate half - lifes at different temperatures without Ea value .

Therefore , answer is (D) , Not enough information has been provided in order to make a conclusion

queen_honey_blossom answered 1 year ago

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