calculate the enthalpy of formation, per mole, of sucrose, C12H2211O(s). C12H22O11(s) + 12O2(g) --> 12CO2(g) +11H2O(l)
deltaH=-5.65*10^3 kJ
To calculate the enthalpy of formation per mole of sucrose (C12H22O11), we need to use the given balanced equation and the enthalpy change (ΔH) value.
The enthalpy of formation (∆Hf) is defined as the change in enthalpy that occurs when one mole of a substance is formed from its elements in their standard states, under standard conditions. For this calculation, we will assume the standard states for the elements are C(graphite), H2(g), O2(g), and H2O(l).
Using the given balanced equation, we can see that 1 mole of sucrose is formed from 12 moles of O2, 12 moles of CO2, and 11 moles of H2O.
The enthalpy change (∆H) for the reaction is given as -5.65x10^3 kJ. This value represents the enthalpy change when the reaction takes place under the specified conditions.
We can use the stoichiometric coefficients from the balanced equation to calculate the enthalpy of formation per mole of sucrose (∆Hf(C12H22O11)).
∆Hf(C12H22O11) = (∆H/12) kJ/mol
Plugging in the given ΔH value:
∆Hf(C12H22O11) = (-5.65x10^3 kJ) / 12 = -470.8 kJ/mol
Therefore, the enthalpy of formation per mole of sucrose (C12H22O11) is approximately -470.8 kJ/mol.
To calculate the enthalpy of formation of sucrose (C12H22O11), we need to use the given balanced chemical equation for the combustion of sucrose and the enthalpy change (deltaH) value.
The equation is:
C12H22O11(s) + 12O2(g) → 12CO2(g) + 11H2O(l)
The enthalpy change (deltaH) for this reaction is -5.65 * 10^3 kJ.
The enthalpy of formation (deltaHf) is the enthalpy change when one mole of a compound is formed from its elements in their standard states.
To calculate the enthalpy of formation of sucrose, we need to consider the enthalpies of formation of carbon dioxide (CO2) and water (H2O). The enthalpy of formation of oxygen (O2) is zero because it is in its standard state.
Using the given equation, we can see that one mole of sucrose produces 12 moles of carbon dioxide and 11 moles of water.
Therefore, the enthalpy of formation of sucrose per mole can be calculated as:
deltaHf (C12H22O11) = (12 moles CO2 x deltaHf(CO2) + 11 moles H2O x deltaHf(H2O)) - (1 mole C12H22O11 x deltaH)
Substituting the given values:
deltaHf (C12H22O11) = (12 * deltaHf(CO2) + 11 * deltaHf(H2O)) - (-5.65 * 10^3 kJ)
Please note that we need the enthalpy of formation values for CO2 and H2O to complete the calculation.