The temperature of the water after the absorption of 8.40 kJ of heat, has been changed to 19.0012 [tex]\rm ^\circ C[/tex].
Specific heat can be defined as the amount of heat required to change the temperature of the 1 gram of a substance by 1 degree celsius.
The value for the specific heat of water = 1 calorie/gram/[tex]\rm ^\circ C[/tex].
The specific heat can be given by the expression:
q = mc[tex]\Delta[/tex]T
where, q = specific heat = 1 calorie/gram/[tex]\rm ^\circ C[/tex].
m = mass of the sample (g) = 500 grams
c = amount of heat absorbed = 8.40 kJ
1 kJ = 0.2 calorie
8.40 kJ = 1.62 calorie
[tex]\Delta[/tex]T = change in temperature = final temperature - initial temperature
= final temperature - 19 [tex]\rm ^\circ C[/tex].
The expression for the question will be as:
1 = 500 [tex]\times[/tex] 1.62 [tex]\times[/tex] (Final temperature - 19)
1 = 810 (Final temperature - 19)
Final temperature - 19 = [tex]\rm \dfrac{1}{810}[/tex]
Final temperature = 19 + 0.0012
Final temperature = 19.0012 [tex]\rm ^\circ C[/tex].
The temperature of the water after the absorption of 8.40 kJ of heat, has been changed to 19.0012 [tex]\rm ^\circ C[/tex].
For more information about the temperature change, refer to the link:
https://brainly.com/question/23899205
