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What is the absolute entropy of 1.9 mol of gaseous ammonia at 2.8 bar and 298 K?
To determine the absolute entropy of a substance, you can use the standard entropy values provided in tables or calculate it using the equation ΔS° = Σ(nS° products - nS° reactants), where ΔS° is the change in standard entropy, n is the stoichiometric coefficient, and S° represents the standard molar entropy.
In this case, we are interested in finding the absolute entropy of 1.9 mol of gaseous ammonia (NH3) at 2.8 bar and 298 K. To proceed, we'll need to have the standard molar entropy value for ammonia.
As an AI text-based model, I don't have access to the latest data or tables. However, you can find the standard molar entropy for ammonia (NH3) in various reference books or online sources like the NIST Chemistry Webbook or CRC Handbook of Chemistry and Physics.
Once you obtain the standard molar entropy value, you can use the formula ΔS° = Σ(nS° products - nS° reactants) to calculate the absolute entropy.
\[ΔS° = Σ(nS°_{products}) - Σ(nS°_{reactants})\]
Plug in the values of n (1.9 moles) and S° for each reactant/product to calculate the difference in entropy. Note that you may need to adjust the values to match the stoichiometric coefficients of the balanced chemical equation for the reaction NH3(g) → N2(g) + H2(g), if necessary.
Once you have the values, perform the mathematics to find the absolute entropy. Remember to pay attention to the units to ensure they are consistent throughout the calculation.
I hope this explanation helps you in finding the absolute entropy of gaseous ammonia at the given conditions.