General Chemistry 2

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$^{-12}$

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.

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$_4$

Balance the redox reaction below

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