Using the following equation for the combustion of octane, calculate the heat associated with the combustion of 100.0 g of octane assuming complete combustion. The molar mass of octane is 114.33 g/mole. The molar mass of oxygen is 31.9988 g/mole.

Using the following equation for the combustion of octane, calculate the heat associated with the combustion of 100.0 g of octane assuming complete combustion. The molar mass of octane is 114.33 g/mole. The molar mass of oxygen is 31.9988 g/mole.

 ΔH°rxn =-11018 kJ

A) -535.4 kJ

B) -4819 kJ

C) -602.3 kJ

D) -385.5 kJ

E) -11018 kJ

 B) -4819 kJ

Explanation:

To calculate the moles :

 ΔH°rxn =-11018 kJ

According to stoichiometry :

2 moles of octane release = 11018 kJ

Thus 0.8747 moles of octane will release =

Heat released is given as negative sign.

Thus the heat associated with the combustion of 100.0 g of octane assuming complete combustion is -4819 kJ

answer: lol

explanation:

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  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-