Chem 1465 1st Edition Lecture 19Outline of Last Lecture 1. Cell notation2. Cell potential A. Galvanic cellsB. Measuring cell potentialC. Standard reduction potentials D. Nonstandard conditions3. Cell potential and equilibrium Outline of Current Lecture1. Possible test questionsCurrent Lecture1. Possible test questionsA. How does entropy change in the following reactions?- A solid melts:- A liquid freezes:- A liquid boils:- A solid sublimes:- A molecule dissolves in water:B. Predict whether the entropy change is positive or negative for the following reactions- 2KClO4(s) → 2KClO3(s) + O2(g) - N2(g) → 2N(g)- 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.C. Given the following equilibrium equation- SO2(g) + Cl2(g) → SO2Cl2(g) , how would the system change if- Cl2(g) was added?- SO2Cl2(g) was removed?- SO2 was removed?D. Consider the 2 equilibrium systems 1) A → 2B ΔH=20KJ, 2) A + B → C ΔH=-5.4KJ. What would happen to equation one and two if- B was removed?- Temperature was increased?E. Identify the bronsted-lowery acid and base, along with the conjugate acid and base - HClO + CH3NH2 → CH3NH3+ + ClO- - CH3COO- + H2O → CH3COOH + OH-- H2PO4- + NH3 → HPO42- + NH4+F. Calculate the pH of a 0.001 M HCl solutionG. For the reaction 2H2(g) + S2(g) → 2H2S(g) , analysis shows that at equilibrium there are 2.5 moles of H2 , 1.35E-5 moles of S2 , and 8.7 moles of H2S in a 12 liter flask. Find
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