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 temperature of the gas, in k, not celsius.

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be