A scientist measures the standard enthalpy change for the following reaction to be -351.2 kJ : P,O10(s) + 6 H,O(1)- →4H3PO (aq) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of P,010(s) is kJ/mol.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![### Problem Statement
A scientist measures the standard enthalpy change for the following reaction to be -351.2 kJ:
\[ \text{P}_4\text{O}_{10}(s) + 6 \text{H}_2\text{O}(l) \rightarrow 4 \text{H}_3\text{PO}_4(aq) \]
Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of \(\text{P}_4\text{O}_{10}(s)\) is:
\[ \_\_\_\_\_\_ \text{kJ/mol} \]
### Answer Submission
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### Notes
- You should derive the enthalpy of formation for \(\text{P}_4\text{O}_{10}(s)\) using the provided enthalpy change and additional standard enthalpies of formation data.
- Make sure your units are consistent and your calculations are precise.
To solve this problem, you'll typically use the given reaction enthalpy, along with the known enthalpies of formation for \(\text{H}_2\text{O}(l)\) and \(\text{H}_3\text{PO}_4(aq)\), applying Hess's Law:
\[ \Delta H_{reaction} = \Sigma \Delta H_f(products) - \Sigma \Delta H_f(reactants). \]
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