General Chemistry 2

What is the solubility of AgCl in 0.020 M NaCN?

AgCl K$_{sp}$ = 1.8 x 10$^{-10}$

Ag(CN)$_2^-$ K$_{f}$ = 5.6 x 10$^{18}$

0.25 moles of AgNO$_3$ are dissolved in 1 L of 0.60 M NaCN and 1 mole of NaCl is added. Will AgCl precipitate?

AgCl K$_{sp}$ = 1.8 x 10$^{-10}$

Ag(CN)$_2^-$ K$_{f}$ = 5.6 x 10$^{18}$

How many moles of Mg(OH)$_2$ can be dissolved in a 1 L solution that already contains 0.52 moles Mg$^{2+}$.

Mg(OH)$_2$ K$_{sp}$ = 8.9 x 10$^{-12}$

The solubility of Ce(IO$_3$)$_3$ in a 0.20 M KIO$_3$ solution is 4.4 x 10$^{-8}$ mol/L. Calculate K$_{sp}$ for Ce(IO$_3$)$_3$.

Calculate the concentrations of Ag$^+$, Ag(S$_2$O$_3$)$^-$, and Ag(S$_2$O$_3$)$_2^{3-}$ in a solution prepared by mixing 150.0 mL of 1.00 x 10$^{-3}$ M AgNO$_3$ with 200.0 mL of 5.00 M Na$_2$S$_2$O$_3$. The stepwise formation equilibria are:

Ag$^+$ + S$_2$O$_3^{2-}$ $\leftrightharpoons$ Ag(S$_2$O$_3$)$^-$ K$_{f1}$ = 7.4 x 10$^{8}$

Ag(S$_2$O$_3$)$^-$ + S$_2$O$_3^{2-}$ $\leftrightharpoons$ Ag(S$_2$O$_3$)$_2^{3-}$ K$_{f2}$ = 3.9 x 10$^{4}$

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

For the reaction above what is $\triangle$H$^\circ$ given that $\triangle$H$_f^\circ$ for NH$_3$ (g) is -45.9 kJ/mol at 25$^\circ$C?

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

For the reaction above, what is the sign and value of entropy for the reaction, given:

H$_2$ (g), S$^\circ$(at 25$^\circ$C) = 130.7 J/(mol*K)

N$_2$ (g), S$^\circ$(at 25$^\circ$C) = 191.56 J/(mol*K)

NH$_3$ (g), S$^\circ$(at 25$^\circ$C) = 192.77 J/(mol*K)

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

For the reaction above, calculate the change in free energy for the reaction, if it were to go to completion.

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

For the reaction above, calculate the free energy of formation, $\triangle$G$_f^\circ$ for each of the products and reactions.

Calculate the standard free energy change, $\triangle$G$^\circ$, for the following reaction. Is the reaction spontaneous?

CH$_4$ (g) + 2 O$_2$ (g) $\longrightarrow$ CO$_2$ (g) + 2 H$_2$O (l)

Values of standard molar entropy, S$_{f}^\circ$ are as follows: CH$_4$ (g), 186 J/(K*mol); O$_2$ (g), 205 J/(K*mol); CO$_2$ (g), 213.6 J/(K*mol); 2 H$_2$O (l), 69.9 J/(K*mol)

$\triangle$H$^\circ$ for this reaction is -890.3 kJ

What is the standard free energy change, $\triangle$G$^\circ$, for the following reaction at 298 K? Is the reaction spontaneous?

2 PCl$_3$ (g) + O$_2$ (g) $\longrightarrow$ 2 POCl$_3$, $\triangle$H = - 620.6 kJ/mol

Values of standard molar entropy, S$_{f}^\circ$ are as follows: 2 PCl$_3$ (g), 311.8 J/K; O$_2$ (g), 205.1 J/K; POCl$_3$, 222.4 J/K

What is the standard free energy change, $\triangle$G$^\circ$, for the following reaction?

Zn (s) + 2 H$^+$ (aq) $\longrightarrow$ Zn$^{2+}$ (aq) + H$_2$ (g), 25$^\circ$C

Standard free energies of formation, $\triangle$G$_{f}^\circ$ are as follows: Zn (s), 0 kJ/mol; 2 H$^+$ (aq), 0 kJ/mol; Zn$^{2+}$ (aq), -147.1 kJ/mol; H$_2$ (g), 0 kJ/mol

Determine the oxidation state of S in Na$_2$SO$_4$

Assign oxidation numbers for the species below. Determine which species is the oxidizing agent and which is the reducing agent. Which species is being oxidized? Which species is being reduced?

Cr$^{3+}$ + Pb $\longrightarrow$ Cr + Pb$^{2+}$

Balance the redox reaction below

Sn + Ag$^+$ $\longrightarrow$ Sn${^2+}$ + Ag

The following reaction takes place under acidic conditions. Assign oxidation numbers and balance the oxidation reduction reaction using the half reaction method.

HNO$_3$ + Fe$^{2+}$ $\longrightarrow$ Fe$^{3+}$ + NO$_2$

Balance the following redox reaction given acidic conditions, using the half reaction method.

$S (s) + NO_2^+ (aq) \longrightarrow SO_2^- (aq) + NO (g)$ .

A voltaic cell is constructed using a Cd/Cd$^{2+}$ half cell and a Sn$^{2+}$/Sn half cell. Write out the balanced equation, determine E$^\circ$, and calculate the cell potential at 25$^\circ$C if [Cd$^{2+}$] = 0.50 M and [Sn$^{2+}$] = 0.30 M.

What is the standard free energy change, $\triangle G ^\circ$ for the following reaction at 25$^\circ$

$Cu ^{2+} (aq) + Fe (s) \longrightarrow Cu (s) + Fe ^{2+} (aq)$

What is the atomic notation for the element Fe?