A certain reaction has an activation energy of 54.0 kJ/mol. As the temperature is increased from 22C to a higher temperature, the rate constant increases by a factor of 7.00. Calculate the higher temperature.

Question

A certain reaction has an activation energy of 54.0 kJ/mol. As the temperature is increased from 22C to a higher temperature, the rate constant increases by a factor of 7.00. Calculate the higher temperature.

Accepted Answer

The higher temperature will be:As the temperature is increased from 22°C to a higher temperature, therateconstant increases by a factor of 7.00. Thefinal temperaturewill be 271.74K.What is the activation energy?Activation energyis defined as the extra energy provided required to activate the molecules to start reacting and forming intermediate and later product.Arrheniusequations given the relation rate constant and activation energy.Where,K= Rate constantA= Pre exponential factorActivation energyWhen two rate constants are givenandGiven,= 22°C = 295KRate constantincreases by a factor of 7,i.e,= 54 kJ/mole = 54000 J/moleR= 8.314Putting the values,ln 7 x 8.31454000 = (1/- 1/295)0.299 x+ 1/295 = 1/0.00368 = 1/= 1/0.00368= 271.74 KTherefore,The increase in temperature will change from 295K to 271.74K.Learn more aboutArrhenius equationof activation here,brainly.com/question/14977272#SPJ4...

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A certain reaction has an activation energy of 54.0 kJ/mol. As the temperature is increased from 22C to a higher temperature, the rate constant increases by a factor of 7.00. Calculate the higher temperature.

A certain reaction has an activation energy of 54.0 kJ/mol. As the temperature is increased from 22C to a higher temperature, the rate constant increases by a factor of 7.00. Calculate the higher temperature.