Jespersen, Chemistry, General Chemistry New Edition (6th) (Chemistry 139 and Che

Question

Jespersen, Chemistry, General Chemistry New Edition (6th) (Chemistry 139 and Chemistry 6e 161) Assignment Gradebook FULL SCREEN PRINTER VERSION 4 BACK NEXT Reaction Rates and Temperature TO4/S04 The reaction HNO2 O3, HNO3 o2, has an activation energy of (-12.31) kj mo 1. At (-23) oc, k 165 L mol 1 s 1. Find the temperature (in K) at which the rate constant will be 61.4 L mol i s i? Round your answer to 3 significant figures. The number of significant digits is set to 3; the tolerance is +/-2% Question Attempts: o of 1 used SAVE FOR LATER SUBMIT ANSWER Copyright o 2000-2014 by John Wiley & Sons, Inc. or related companies. All rights reserved.

Explanation / Answer

by applying arrhenius equation, k = Ae-Ea/RT , where , k= rate constant , Ea=activation energy , R=gas constant, T=temperature

in 1st case , T=273-23 K = 250 K , Ea=-12.31KJ/mol , k = 165L/mol s , putting these values in the above values , we get the only unknown value of A as 0.442

now , in 2nd case , A=0.442 , Ea = -12.31KJ/mol , k=61.4L/mol s , by putting all these values in the arrhenius equation , we get , T = 300K , so the required temperature is 300K

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