ThermochemistryHard
Question
When 1.0 g of oxalic acid (H2C2O4) is burned in a bomb calorimeter whose heat capacity is 8.75 kJ/K, the temperature increases by 0.312 K. The enthalpy of combustion of oxalic acid at 27oC is :
Options
A.-245.7 kJ/mol
B.-244.452 kJ/mol
C.-246.947 kJ/mol
D.None of these
Solution
H2C2O4(l) + 
O2(g) → H2O(l) + 2CO2(g);
ᐃng = 3/2
ᐃUc = -
× 90
= - 245.7 kJ/mol
ᐃH = ᐃU + ᐃngRT
= - 245.7 +
= - 246.947 kJ/mol
O2(g) → H2O(l) + 2CO2(g);ᐃng = 3/2
ᐃUc = -
× 90= - 245.7 kJ/mol
ᐃH = ᐃU + ᐃngRT
= - 245.7 +
= - 246.947 kJ/molCreate a free account to view solution
View Solution FreeMore Thermochemistry Questions
Assume that for a domestic hot water supply, 160 kg of water per day must be heated from 10oC to 60oC and gaseous fuel p...A solution was prepared by dissolving 7.45 g of KCl in 200 g of H2O in a calorimeter with a water equivalent of 25 g. Th...ᐃHfo(298K) of methanol is given by the chemical equation :...The most exothermic ‘ordinary’ chemical reaction for a given mass of reactants is 2H(g) → H2(g), where ΔE = 103 kcal. Th...ΔfH° for CO2(g) and H2O(l) are −94.0 and −68.0 kcal/mol. ΔfH° for the propanoic acid is one-third of the enthalpy of com...