The graph above shows the changes in temperature recorded for the 2.00 l of h2o surrounding a constant-volume container in which

Answer:

25.2 kJ

Explanation:

The full question can be found in the image linked to this response.

It's important to highlight that the heat absorbed by the 2.00 L of water for increasing its temperature from the beginning to the end comes solely from the burning of benzoic acid, as there are no heat transfers to the container or the surroundings.

To find the heat released from benzoic acid combustion, we simply measure the heat needed to warm the water.

Q = mCΔT

To find the mass of the water,

Density = (mass)/(volume)

Mass = Density × volume

Density = 1 g/mL

Volume = 2.00 L = 2000 mL

Mass = 1 × 2000 = 2000 g

C = specific heat of water = 4.2 J/g.°C

ΔT = (final temperature) - (Initial temperature)

Final water temperature = 25°C

Initial water temperature = 22°C

ΔT = 25 - 22 = 3°C

Q = (2000×4.2×3) = 25,200 J = 25.2 kJ

Hope this Helps!!!