The balanced combustion reaction for C 6 H 6 C6H6 is 2 C 6 H 6 ( l ) + 15 O 2 ( g ) ⟶ 12 CO 2 ( g ) + 6 H 2 O ( l ) + 6542 kJ 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6 542 kJ If 7.300 g C 6 H 6 7.300 g C6H6 is burned and the heat produced from the burning is added to 5691 g 5691 g of water at 21 ∘ 21 ∘ C, what is the final temperature of the water?

The final temperature of the water is .

Explanation:

We know that molar mass of is 78 g/mol. And, the amount of heat produced when 2 mol of burns is 6542 KJ.

This means that,

    = 156 g of burns, heat produced is 6542 kJ.

Therefore, heat produced (Q) by burning  7.3 g of is as follows.

              = 306.13 kJ

or,           = 306130 J      (as 1 KJ = 1000 J)

For water, mass is given as 5691 g and specific heat capacity of water is 4.186 .

So, we will calculate the value of final temperature as follows.

            Q =

  306130 J =

          = 12.85 + 21

                      =

Thus, we can conclude that the final temperature of the water is .

the answer is option a.