The balanced combustion reaction for c 6 h 6 is 2 c 6 h 6 ( l ) 15 o 2 ( g ) ⟶ 12 co 2 ( g ) 6 h 2 o ( l ) 6542 kj if 7.700 g c 6 h 6 is burned and the heat produced from the burning is added to 5691 g of water at 21 ∘ c, what is the final temperature of the water

Explanation:

To calculate the moles, we use the equation:

According to stoichiometry :

2 moles of releases = 6542 kJ of heat

0.9858 moles of  release = of heat

Thus heat given off by burning 7.700 g of  will be absorbed by water.

Q = Heat absorbed= 3224kJ = 3224000J   (1kJ=1000J)

m= mass of water = 5691 g

c = specific heat capacity =

Initial temperature of the water = = 21.0°C

Final temperature of the water =  = ?

Putting in the values, we get:

The final temperature of the water is

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.