To calculate the deltaS(sys), you need to use the change in entropy values for each species involved in the reaction. The change in entropy values can be found from tables or calculated using the formula:
deltaS = n * deltaS°(products) - m * deltaS°(reactants)
Where:
- deltaS is the change in entropy
- n and m are the stoichiometric coefficients of the products and reactants
- deltaS° is the standard entropy change for each species
Using the values you provided, the calculation for deltaS(sys) can be done as follows:
deltaS(sys) = (1 * 214.4) - (1 * 0 + 2 * 223.1)
= 214.4 – 446.2
= -231.8 J/mol*K
Therefore, the correct value for deltaS(sys) is -231.8 J/mol*K, not -253.3 J/mol*K as stated in your answer.
To calculate deltaS(surr), we can use the equation:
deltaS(surr) = -deltaH(sys) / T
Where:
- deltaH(sys) is the enthalpy change of the system (given as -139 kJ/mol)
- T is the temperature in Kelvin (298 K)
deltaS(surr) = -(-139 kJ/mol) / (298 K)
= 466.4 J/mol*K
Therefore, the value for deltaS(surr) is indeed 466.4 J/mol*K.
Lastly, to calculate deltaS(univ), it can be done using the equation:
deltaS(univ) = deltaS(sys) + deltaS(surr)
deltaS(univ) = -231.8 J/mol*K + 466.4 J/mol*K
= 234.6 J/mol*K
Therefore, the correct value for deltaS(univ) is 234.6 J/mol*K, not 231.4 J/mol*K as stated in your answer.
I hope this helps clarify the calculation and provides you with the correct values for deltaS(sys), deltaS(surr), and deltaS(univ).