Question
The enthalpy change for 2KClO3 = 2KCl +3O2
Answers
GPT 3.5
To calculate the enthalpy change for the given reaction, we need to consider the enthalpy values of the reactants and products.
The balanced equation for the reaction is:
2KClO3 → 2KCl + 3O2
Given:
- The enthalpy change of formation for KClO3 (ΔHf°) = -395 kJ/mol
- The enthalpy change of formation for KCl (ΔHf°) = -436 kJ/mol
- The enthalpy change of formation for O2 (ΔHf°) = 0 kJ/mol (since it is an element in its standard state)
The enthalpy change (ΔH) for the reaction can be calculated using the following formula:
ΔH = ∑(nΔHf° products) - ∑(nΔHf° reactants)
Where n is the stoichiometric coefficient of each species in the balanced equation, and ΔHf° is the standard heat of formation.
For the reactants:
ΔH = (2mol)(-436 kJ/mol) + (3mol)(0 kJ/mol) - (2mol)(-395 kJ/mol)
= -872 kJ/mol + 0 kJ/mol + 790 kJ/mol
= -82 kJ/mol
Therefore, the enthalpy change (∆H) for the given reaction is -82 kJ/mol.
The balanced equation for the reaction is:
2KClO3 → 2KCl + 3O2
Given:
- The enthalpy change of formation for KClO3 (ΔHf°) = -395 kJ/mol
- The enthalpy change of formation for KCl (ΔHf°) = -436 kJ/mol
- The enthalpy change of formation for O2 (ΔHf°) = 0 kJ/mol (since it is an element in its standard state)
The enthalpy change (ΔH) for the reaction can be calculated using the following formula:
ΔH = ∑(nΔHf° products) - ∑(nΔHf° reactants)
Where n is the stoichiometric coefficient of each species in the balanced equation, and ΔHf° is the standard heat of formation.
For the reactants:
ΔH = (2mol)(-436 kJ/mol) + (3mol)(0 kJ/mol) - (2mol)(-395 kJ/mol)
= -872 kJ/mol + 0 kJ/mol + 790 kJ/mol
= -82 kJ/mol
Therefore, the enthalpy change (∆H) for the given reaction is -82 kJ/mol.
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