Respuesta :
Explanation:
First, we will calculate the molar mass of [tex]C_{6}H_{6}[/tex] as follows.
Molar mass of [tex]C_{6}H_{6}[/tex] = [tex]6 \times 12 + 6 \times 1[/tex]
= 78 g/mol
So, when 2 mol of [tex]C_{2}H{6}[/tex] burns, then heat produced = 6542 KJ
Hence, this means that 2 molecules of [tex]C_{6}H{6}[/tex] are equal to [tex]78 \times 2 = 156 g[/tex] of [tex]C_{6}H_{6}[/tex] burns, heat produced = 6542 KJ
Therefore, heat produced by burning 5.5 g of [tex]C_{6}H{6}[/tex] =
[tex]6542 kJ \times \frac{5.5 g}{156 g}[/tex]
= 228.97 kJ
= 228970 J (as 1 kJ = 1000 J)
It if given that for water, m = 5691 g
And, we know that specific heat capacity of water is 4.186 [tex]J/g^{o}C[/tex] .
As, Q = [tex]m \times C \times (T_{f} - T_{i})[/tex]
228970 J = [tex]5691 g \times 4.184 J/g^{o}C \times (T_{f} - 21) ^{o}C[/tex]
[tex]T_{f} - 21^{o}C = 9.616^{o}C[/tex]
[tex]T_{f} = 30.6^{o}C[/tex]
Thus, we can conclude that the final temperature of the water is [tex]30.6^{o}C[/tex].
