In: Chemistry
Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It metls at -73.0 degrees Celsius and boils at -10.0 degrees celsius. Its change enthalpy (fusion) is 8.619 kJ/mol, and its change in enthalpy (vaporization) is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g.K and 0.622J/g.K, respectively. How much heat is required to convert 2.750kg of solid SO2 at the metling point to a gas at 60.0 degrees Celsius?
Four steps in the calculation of heat
1. To melt the So2 at its melting point
2. To heat the liquid SO2 upto its boiling point
3. To evaporate So2 at its boiling point
4. To heat So2 gas upto 60C
1. Q1 = n* H fuion
Where n is no of moles of SO2 = 2750/64
= 42.96875 moles
Q1 = 42.96875*8.619 = 370.64Kj
2. Q2 = m*C* ∆T
m= mass of SO2 = 2750gm
C= Specific haet capacity of SO2 =
0.995j/k.g
∆T = temperature difference -10-(-73) =63C
Q2 = 2750*0.995*63 = 172.383Kj
3. Q3 = n*H vapor
= 42.96875*25.73
= 1105.58Kj
4. Q4 = m*C* ∆T
m = mass of SO2 = 2750g
C = specific heat capacity of SO2 =
0.622j/gk
∆T = Temperature = 60-(10) = 70C
Q4 = 2750*0.622*70
= 119.735kj
Total heat required
Q = Q1+Q2+Q3+Q4
= 370.64+172.383+1105.58+119.735
= 1768.338kj