Using the following equation for the combustion of octane, calculate the heat associated with the formation of 100.0 g of carbon dioxide. The molar mass of octane is 114.33 g/mol. The molar mass of carbon dioxide is 44.0095 g/mol.

Heat associated with the formation of 100.0 g of carbon dioxide is 1563.2 kJ.

Explanation:

Reaction equation will be as follows.

    ;   = -11018 kJ

Mass of = 100 g

Hence, moles of present will be calculated as follows.

       No. of moles =

                             =

                             = 2.27 mol

Therefore, heat produced by 2.27 mol for the given reaction will be calculated as follows.

             = 1563.2 kJ

Thus, we can conclude that heat associated with the formation of 100.0 g of carbon dioxide is 1563.2 kJ.

here we have to get the change of moles on decrease the volume of the reaction in gas phase.

the   per the given options it will decrease by (d) 11-50%

we know, on decreasing the volume of the gas phase reaction the reaction moves to the product side.

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:                   1 - α               α               α           = 1 + α

(concentration = moles/volume, as volume is 1 l)

(where α is the degree of dissociation)

now the dissociation constant in terms of concentration is :

=  

or,

or,   = (at v = 1l)

the reaction:                     so₂cl₂ (g) = so₂ (g) + cl₂ (g)         total

the moles at equilibrium:   1 - α                 α               α           = 1+α

concentrations:               (1 - α)/0.5           α/0.5         α/0.5       = (1 + α)/0.5

thus, the dissociation constant in terms of concentration is :

or,  

=  

so, the change of 1 : 1/0.5

or, 1: 2

thus it will decrease by 50%.

or, as per the given options it will decrease by 11-50%