The activation energy of a certain reaction is 40.1 kj/mol . at 26 ∘c , the rate constant is 0.0160s−1. at what temperature in degrees celsius would this reaction go twice as fast? express your answer with the appropriate units. view available hint(s)

Explanation:

We can use the Arrhenius equation:

Data:

Eₐ = 40.1 kJ·mol⁻¹

k₁ = 0.0160 s⁻¹;              k₂ = 0.0320 s⁻¹

T₁ = 26 °C = 299.15 K; T₂ = ?  

Calculations:

T₂ = 312.6 K = 39 °C

The reaction will go twice as fast at .

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :