Write the balanced K, and K, reactions for HSo, in K.:

An instant cold pack purchased in a pharmacy contains a packet of solid ammonium nitrate surrounded by a pouch of water. When the packet of NH4NO3 is broken, the solid dissolves in water and cooling of the mixture occurs because the solution process for NH4NO3 is endothermic. Explain, in terms of what happens to the molecules and ions, why this mixing occurs spontaneously. Select all that apply. In solution, the ions NH4* and NO3 are highly ordered throughout the solvent. In the solid, the ions in NH4NO3 are highly ordered. In solution, the ions NH4+ and NO3 are randomly distributed throughout the solvent. The increase in randomness makes the process spontaneous. The decrease in randomness makes the process spontaneous.

4. An experiment is to be performed to determine the standard molar enthalpy of neutralization of a  strong acid by a strong base. Standard school laboratory equipment and a supply of standardized 1.00  mol/L HCl and standardized 1.00 mol/L NaOH are available.   a. What equipment would be needed? List them. b. What measurements should be taken? List them.  c. Without performing calculations, briefly describe how the resulting data should be used to  obtain the standard molar enthalpy of neutralization.  d. When a class of students performed this experiment, the average of the results was -55.0  kJ/mol. The accepted value for the standard molar enthalpy of neutralization of a strong acid by  a strong base is -57.7 kilojoules per mole. Briefly describe two likely sources of experimental error that could account for the result  obtained by the class. Mistakes, blunders, or miscalculations are not types of experimental error.

4. Write a dissociation equation for the following: a) CaCl b) Al-(SO.)x0).

Predict the reaction. Explain briefly.

5. If magnesium hydroxide were used instead of NaOH, how many moles would it take to combine with three moles of KHP? Explain.

Calculate the lattice energy of AgBr(s) using the following thermodynamic data (all data is in kJ/mol).  Ag(s) ΔHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Br-Br(g) Bond energy = 173 kJ/mol Br(g) Electron affinity = -345 kJ/mol AgBr(s) ΔH°f = -120 kJ/mol ______________ kJ/mol

7. NaCl(ag) +

Write the balanced equation for each reaction. Phases are optional. The carbonate ion (CO) acts as a Brønsted base with water. equation: The carbon-containing product from the first reaction acts as a Brønsted base with water. equation: The carbon-containing product from the second reaction decomposes into carbon dioxide gas and water. equation: Consider the products of the reactions. When the carbonate ion reacts with water, is the resulting solution acidic or basic? basic acidic

Give detailed Solution with explanation needed (no need Handwritten