ThermochemistryHard
Question
The heat of reaction for : C10H8(s) + 12O2(g) → 10CO2(g) + 4H2O(l) at constant volume is 1228.2 kcal at 25oC. The heat of reaction at contant pressure and same temperature is :
Options
A.-1228.2 kcal
B.-1229.3 kcal
C.-1232.9 kcal
D.1242.6 kcal
Solution
ᐃE = - 1228.2Kcal = 1228.2 × 103cal
ᐃH = ᐃE + ᐃnRT
1228.2 × 103 = (-2)(2)(298)
= - 1229392 cal
= - 1229.392 kcal
ᐃH = ᐃE + ᐃnRT
1228.2 × 103 = (-2)(2)(298)
= - 1229392 cal
= - 1229.392 kcal
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
For a specific work, on an average a person requires 5616 kJ of energy. How many kilograms of glucose must be consumed i...Tungsten carbide is very hard and is used to make cutting tools and rock drills. What is the enthalpy of formation (in k...If the enthalpy of formation and enthalpy of solution of HCl (g) are - 92.3 kJ/mol and - 75.14 kJ/mol respectively then ...Enthalpy of neutralisation of CH3COOH by NaOH is - 50.6 kJ/mol and the heat of neutralisation of a strong acid with NaOH...Calculate the enthalpy of formation of I2O5(s) from the following data.(i) I2O5(s) + H2O(l) → 2HIO3(aq): ΔH = +4.0 kJ(ii...