The reaction c4h8(g)⟶2c2h4(g) c4h8(g)⟶2c2h4(g) has an activation energy of 262 kj/mol.262 kj/mol. at 600.0 k,600.0 k, the rate constant, , is 6.1×10−8 s−1.6.1×10−8 s−1. what is the value of the rate constant at 785.0 k?

Answer : The rate constant at 785.0 K is,

Explanation :

According to the Arrhenius equation,

or,

where,

= rate constant at =

= rate constant at = ?

= activation energy for the reaction = 262 kJ/mole = 262000 J/mole

R = gas constant = 8.314 J/mole.K

= initial temperature =

= final temperature =

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

Therefore, the rate constant at 785.0 K is,

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.