Respuesta :
You have to use the equation q=mcΔT and solve for T(final).
T(final)=(q/mc)+T(initial)
q=the amount of energy absorbed or released (in this case 868J)
m=the mass of the sample (in this case 15.6g)
c= the specific heat capacity of the substance (in this case 2.41 J/g°C)
T(initial)=the initial temperature of the sample (in this case 21.5°C)
When you plug everything in, you should get 44.6°C.
Therefore the final temperature of ethanol is 44.6°C
I hope this helps. Let me know if anything is unclear.
T(final)=(q/mc)+T(initial)
q=the amount of energy absorbed or released (in this case 868J)
m=the mass of the sample (in this case 15.6g)
c= the specific heat capacity of the substance (in this case 2.41 J/g°C)
T(initial)=the initial temperature of the sample (in this case 21.5°C)
When you plug everything in, you should get 44.6°C.
Therefore the final temperature of ethanol is 44.6°C
I hope this helps. Let me know if anything is unclear.
The final temperature of the ethanol is 44.6°C.
Given:
- The 15.6 grams of ethanol absorbs 868 Joules of energy on heating.
- The initial temperature of the ethanol was 21.5°C.
- The specific heat of ethanol is 2.41 J/g°C
To find:
The final temperature of the ethanol.
Solution:
The mass of ethanol = m = 15.6 g
The specific heat of an ethanol = c = 2.41 J/g°C
The initial temperature of the ethanol = [tex]T_1=21.5^oC[/tex]
The final temperature of the ethanol = [tex]T_2=?[/tex]
The amount heat added to ethanol= Q = 868 J
The amount of heat added to a substance is given by the equation:
[tex]Q=m\times c\times (T_2-T_1)\\\\868 J=15.6 g\times 2.41 J/g^oC\times (T_2-21.5^oC)\\\\\frac{868 J}{15.6 g\times 2.41 J/g^oC}=(T_2-21.5^oC)\\\\T_2=\frac{868 J}{15.6 g\times 2.41 J/g^oC}+21.5^oC\\\\=44.6 ^oC[/tex]
The final temperature of the ethanol is 44.6°C.
Learn more about the specific heat of substance here:
brainly.com/question/16735503?referrer=searchResults
brainly.com/question/1209542?referrer=searchResults
