The balanced combustion reaction for c6h6 is 2c6h6(l)+15o2(g)⟶12co2(g)+6h2o(l)+6 542 kj if 8.600 g c6h6 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?

Answer : The final temperature of the water is,

Explanation : Given,

Mass of benzene = 8.600 g

Molar mass of benzene = 78 g/mole

First we have to calculate the moles of benzene.

Now we have to calculate the energy of combustion.

The given balanced chemical reaction is:

According to reaction,

As, 2 moles of benzene gives 6542 kJ of energy on combustion.

So, 0.1103 mole of benzene gives of energy on combustion.

Now we have to calculate the final temperature of the water.

Formula used :

where,

= heat released = 360.7913 kJ = 36079.13 J

= mass of water = 5691 g

= specific heat of water=

= final temperature = ?

= initial temperature =

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

Therefore, the final temperature of the water is,

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.

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