consider the following reaction at 298K
4Al(s)+3O2(g) yields 2Al2O3(s)
delta H= -3351.4 Kj
find delta S sys
find delta S surr
find delta S unvi
To find the entropy change for the system (ΔSsys), the entropy change for the surroundings (ΔSsurr), and the total entropy change (ΔSuniv), you can use the following equations:
ΔSsys = (ΔHsys) / T
ΔSsurr = (-ΔHsys) / T
ΔSuniv = ΔSsys + ΔSsurr
where:
ΔHsys is the enthalpy change of the system
T is the temperature in Kelvin
Given:
ΔH = -3351.4 kJ
Step 1: Convert ΔH from kJ to J
ΔH = -3351.4 kJ × 1000 J/1 kJ = -3351400 J
Step 2: Calculate ΔSsys using the equation:
ΔSsys = (ΔHsys) / T = (-3351400 J) / 298 K = -11245 J/K
Step 3: Calculate ΔSsurr using the equation:
ΔSsurr = (-ΔHsys) / T = (-(-3351400 J)) / 298 K = 11245 J/K
Step 4: Calculate ΔSuniv using the equation:
ΔSuniv = ΔSsys + ΔSsurr = (-11245 J/K) + (11245 J/K) = 0
Therefore, the values are:
ΔSsys = -11245 J/K
ΔSsurr = 11245 J/K
ΔSuniv = 0 J/K