Respuesta :
Explanation:
As we know that specific heat is the amount of energy required to raise the temperature by [tex]1^{o}C[/tex]. So here, specific heat is given as 3.85 J. And, the change in temperature is [tex]14.6^{o}C[/tex].
Therefore, we will calculate the heat energy as follows.
q = [tex]C \times \Delta T[/tex]
= [tex]3.85 J \times 14.6^{o}C[/tex]
= 56.21 [tex]J^{o}C[/tex]
Since, it is given that heat released for 1 mole\ is 480 kJ or 48000 J (as 1 kJ = 1000 J). Therefore, moles required to produce 56.21 [tex]J/^{o}C[/tex] of heat is calculated as follows.
[tex]\frac{56.21 J/^{o}C}{48000 J^{o}C}[/tex]
= [tex]1.17 \times 10^{-3}[/tex] moles
Thus, we can conclude that number of moles of reactant that were consumed are [tex]1.17 \times 10^{-3}[/tex] moles.
