If 8.800 g of 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?

Before we solve for the final temperature, the initial temperature should be given. Suppose this is at room temperature, 25°C. The solution is as follows.

8.8 g (1/Molar mass of benzene) (Heat of combustion of benzene) = 5,691 g water (Heat capacity of water) (Tfinal - Tinitial)

Heat from benzene = - Heat from water

8.8 g (1/78 g/mol) (-3,271 kJ/mol) = - (5,691 g) (4.816 J/g·°C) (1 kJ/1000 J) (Tfinal - 25°C)

Tfinal = 38.46°C