Part A - Calculating ΔS∘ from Tabulated Entropies Using the standard molar entropies below, calculate the standard entropy chang
e, ΔS∘ , for the "water-splitting" reaction at 298 K: 2H2O(l) → 2H2(g) + O2(g) Standard Molar Entropies of Selected Substances at 298 K Substance S∘ (J/mol⋅K) H2(g) 130.6 O2(g) 205.0 H2O(g) 188.8 H2O(l) 69.9 Using the standard molar entropies below, calculate the standard entropy change, , for the "water-splitting" reaction at 298 : Standard Molar Entropies of Selected Substances at 298 Substance () 130.6 205.0 188.8 69.9 326.4 J/K 265.7 J/K 163.2 J/K 88.5 J/K −326.3 J/K
Titration curves for strong and weak acids illustrating the proper choice of acid-base indicator. Any of the three indicators will exhibit a reasonably sharp color change at the equivalence point of the strong acid titration, but only phenolphthalein is suitable for use in the weak acid titration.
2) HClO3 is stronger because chlorine is more electronegative than iodine.
Explanation:
The more electronegative the element is the more strong or acidic it becomes.
Chlorine being more electronegative than Iodine makes it easier for it to pull the electron of hydrogen more strongly and hence has a higher tendency to release a H+ unit. Hence that makes it stronger.