Answer : The amount of in kilojoules released is, -5.53 kJ
Explanation :
Formula used :
[tex]q=m\times c\times (T_{final}-T_{initial})[/tex]
where,
q = heat released = ?
c = specific heat of ethanol = [tex]2.41J/g^oC[/tex]
m = mass of ethanol = 23.4 g
[tex]T_{final}[/tex] = final temperature = [tex]-15.0^oC[/tex]
[tex]T_{initial}[/tex] = initial temperature = [tex]83.0^oC[/tex]
Now put all the given values in the above formula, we get:
[tex]q=23.4g\times 2.41J/g^oC\times (-15.0-83.0)^oC[/tex]
[tex]q=-5526.612J=-5.53\times 10^3J=-5.53kJ[/tex]
Therefore, the amount of in kilojoules released is, -5.53 kJ
