The heat of combustion for solid citric acid (C6H8O7) is quantified as ΔH = -1986 kJ/mol at 298 K. To calculate the heat liberated from the combustion of 10g of citric acid, one must first convert the mass into moles using the molar mass of citric acid, which is approximately 192.13 g/mol. The total heat released can then be determined by multiplying the number of moles by the heat of combustion per mole. This calculation is performed at constant pressure, which is standard for combustion reactions, making pressure specification unnecessary.
PREREQUISITESChemistry students, chemical engineers, and professionals involved in energy calculations or combustion analysis will benefit from this discussion.
rcs said:I am confused on how to find out the heat of combustion of solid citric acid to water and carbondioxide that is deltaH 296 -1986 kJ/mol. I need to figure out the heat liberated when 10g of citric acid is totally combusted at 298k? *a) At constant pressure?? at constant volume?? and why is it not necessary to specify the pressure in part a?