Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at -73°C and boils at -10°C. Its H°fus is 8.619 kJ/mol and its H°vap is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g·K and 0.622 J/g·K, respectively. How much heat is required to convert 2.490 kg of solid SO2 at the melting point to a gas at 60°C?
2007-12-03 02:16:59 · 1 answers · asked by jnester0289 1 in Science & Mathematics ➔ Chemistry
molar mass of SO2 is 32+2*16=64g
so 2.490 kg = 2490/64 =38.91moles
first step melt the SO2 at -73 H1 = 38.91*8.619 =335.33 kJ
second step warm from -73°C to -10°C
H2 = mc(Tf-Ti) =2490*0.995*(-10-(-73)) =2490*0.995*63=156086J= 156.086kJ
third step evaporate SO2
H3= 38.91*25.73=1001.15kJ
fourth step warm gas from -10°C to 70°C
H4 = 2490*0.622*(60-(-10)) =108,415J =108.415kJ
so total amount of heat =
H1+H2+H3+H4 =335.33+156.086+1001.15+108.415=1601kJ (at 0.1kJ)
2007-12-03 02:54:15 · answer #1 · answered by maussy 7 · 0⤊ 0⤋