Answer:
4739.86 J/mol.
Step-by-step explanation:
The amount of heat released to water = Q = m.c.ΔT.
where, m is the mass of water (m = 367.0 g).
c is the specific heat capacity of water = 4.18 J/g°C.
ΔT is the temperature difference = (final T - initial T = 87.0°C - 24.0°C = 63.0°C).
∴ The amount of heat absorbed by released to water = Q = m.c.ΔT = (367.0 g)(4.18 J/g°C)(63.0°C) = 96645.78 J.
- Since, the reaction releases heat, so the reaction is exothermic (ΔH is negative).
ΔH = Q/n.
n = mass/molar mass = 367 g/18 g/mol = 20.39 mol.
∴ ΔH = Q/n = - (96645.78 J)/(20.39 mol) = 4739.86 J/mol.