Calculate the change in entropy. enthalpy and Gibbs energy under standard conditions for the reaction of the formation of glycine
CH3 (NH2)COOH1>CH2(NH2)CONHCH2COOH1+H2O1.298 k
glycine
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To calculate the change in entropy, enthalpy, and Gibbs energy for the reaction of the formation of glycine (CH3(NH2)COOH), you will need the standard entropy, enthalpy, and Gibbs energy values for each of the reactants and products involved in the reaction.
1. Start by writing the balanced equation for the reaction:
CH3(NH2)COOH (s) → CH2(NH2)CONHCH2COOH (s) + H2O (l)
2. Look up the standard entropy (∆S°) values for each compound involved in the reaction. The standard entropy is usually given in units of J/(mol·K) and is denoted by the symbol ∆S°.
3. Calculate the change in entropy (∆S°) for the reaction using the following equation:
∆S° = ΣS°(products) - ΣS°(reactants)
Replace ΣS°(products) with the sum of the standard entropy values of the products and ΣS°(reactants) with the sum of the standard entropy values of the reactants.
4. Similarly, look up the standard enthalpy (∆H°) values for each compound involved in the reaction. The standard enthalpy is usually given in units of kJ/mol and is denoted by the symbol ∆H°.
5. Calculate the change in enthalpy (∆H°) for the reaction using the following equation:
∆H° = ΣH°(products) - ΣH°(reactants)
Replace ΣH°(products) with the sum of the standard enthalpy values of the products and ΣH°(reactants) with the sum of the standard enthalpy values of the reactants.
6. Use the standard Gibbs energy (∆G°) equation to calculate the change in Gibbs energy for the reaction:
∆G° = ∆H° - T∆S°
where ∆H° is the change in enthalpy calculated previously, ∆S° is the change in entropy calculated previously, and T is the temperature of the reaction in Kelvin.
Be sure to use consistent units when plugging numbers into the equations. Consult reliable sources such as textbooks or databases for accurate values of standard entropy, enthalpy, and Gibbs energy.