ΔH° = +178 kJ/mol
How much heat must be absorbed by 43.0 g of CaCO3 to convert it completely to CaO?
can someone explain this?
Convert 43.0 g into moles of CaCO3, and multiply it by the enthalpy.
43.0 g / 100.0869 g/mol = 0.430 mol
0.430 mol x 178 kJ/mol = 76.5 kJ
The enthalpy gives you how much heat is transferred per mole, so first find the moles and multiply it by the enthalpy.
if the -6278kJ is the warmth of the reaction as written, ie for the combustion of two moles benzene then combustion of two x seventy 8.11g produces 6278kj or 24.3 g produces (6278/(2 x seventy 8.11)) x 24.3 = 976.5 kJ
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Convert 43.0 g into moles of CaCO3, and multiply it by the enthalpy.
43.0 g / 100.0869 g/mol = 0.430 mol
0.430 mol x 178 kJ/mol = 76.5 kJ
The enthalpy gives you how much heat is transferred per mole, so first find the moles and multiply it by the enthalpy.
if the -6278kJ is the warmth of the reaction as written, ie for the combustion of two moles benzene then combustion of two x seventy 8.11g produces 6278kj or 24.3 g produces (6278/(2 x seventy 8.11)) x 24.3 = 976.5 kJ