Answer:
25.2 kJ
Explanation:
The complete question is presented in the attached image to this answer.
Note that, the heat gained by the 2.00 L of water to raise its temperature from the initial value to its final value comes entirely from the combustion of the benzoic acid since there are no heat losses to the containing vessel or to the environment.
So, to obtained the heat released from the combustion of benzoic acid, we just calculate the heat required to raise the temperature of the water.
Q = mCΔT
To calculate the mass of 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 capacity of water = 4.2 J/g.°C
ΔT = (final temperature) - (Initial temperature)
From the graph,
Final temperature of water = 25°C
Initial temperature of water = 22°C
ΔT = 25 - 22 = 3°C
Q = (2000×4.2×3) = 25,200 J = 25.2 kJ
Hope this Helps!!!
Specific heat is defined as the heat needed to raise the temperature of the unit mass of a given substance.
The specific heat is calculated by:
Q = mc[tex]\Delta[/tex]T
The heat released from the combustion of benzoic acid sample is 25.2 kJ.
The heat gained by 2.00 L water to raise the temperature from initial to final value is derived from the combustion of benzoic acid.
Since, there is no loss of heat to the environment, then:
Q = mc[tex]\Delta[/tex]T
Also,
Density = mass/ volume
Mass = Density x volume
Given,
Volume = 2 L
Mass = 2000 g
Specific heat = 4.2 J/g.°C
[tex]\Delta[/tex]T = Initial -final = 25 - 22 = 3°C
Thus, the value for Q can be calcuated as:
Q = (2000×4.2×3) = 25,200 J = 25.2 kJ
Therefore, the heat released is equal to 25.2 KJ.
To know more about specific heat, refer to the following link:
https://brainly.com/question/11297584