The gas phase reaction 2 N2O5(g) → 4 NO2(g) + O2(g) has an activation energy of 103 kJ/mol, and the first order rate constant is 1.35×10-5 min-1 at 266 K. What is the rate constant at 296 K?

 The rate constant at 296 K is

Explanation:

According to the Arrhenius equation,

or,

where,

= rate constant at 266 K =

= rate constant at 296 K = ?

= activation energy for the reaction = 103 kJ/mol = 103000 J/mol

R = gas constant = 8.314 J/mole.K

= initial temperature = 266 K

= final temperature = 296 K

Now put all the given values in this formula, we get

Thus the rate constant at 296 K is

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer