Consider the decomposition of barium carbonate:

$$\ce{BaCO3(s) <=> BaO(s) +CO2(g)}$$

Using data from Appendix C in the textbook, calculate the equilibrium pressure of CO2 at

(a) 298 K
(b) 1100 K

Using data in Appendix E in the textbook, calculate the standard emf for each of the following reactions:

a) $\mathrm{H_2(g)+F_2(g)\rightarrow 2H+(aq)+2F^−(aq)}$

b)$\mathrm{ Cu_2+( aq )+Ca(s)\rightarrow Cu(s)+Ca^{2+}(aq)}$

c) $\mathrm{2ClO_3^-( a q )+10Br^-(aq)+12H^+(aq)\rightarrow Cl_2( g )+5Br_2(l)+6H_2O(l)}$

The following equilibrium constants were determined at $1123 \mathrm{~K}$ :

$$\begin{array}{lll} \mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}) & & \\ \\ K_P=1.3 \times 10^{14} \\ \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{COCl}_2(\mathrm{~g}) & \\ K_P=1.3 \times 10^{14} \\ & & \\ & & \end{array}$$

Write the equilibrium constant expression $K_p$, and calculate the equilibrium constant at $1123 \mathrm{~K}$ for

$$\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})+2 \mathrm{Cl}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{COCl}_2(\mathrm{~g})$$

.

Write the equilibrium-constant expression and calculate the value of the equilibrium constant for each of the following reactions at $298 \mathrm{~K}$, using data from Appendix C:

$$2 \mathrm{HBr}(g)+\mathrm{Cl}_2(g) \rightleftharpoons 2 \mathrm{HCl}(g)+\mathrm{Br}_2(g)$$

A student placed 1 g of each of three compounds A, B, and C in a container and found that after 1 week no change had occurred. Offer some possible explanations for the fact that no reactions took place. Assume that A, B, and C are totally miscible liquids.

Consider the decomposition of barium carbonate:

$$\mathrm{BaCO}_3(\mathrm{~s}) \rightleftharpoons \mathrm{BaO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$$

Using data from Appendix C, calculate the equilibrium pressure of $\mathrm{CO}_2$ at

$1100 \mathrm{~K}$.

Consider the following reaction:

$$\mathrm{PbCO}_3(\mathrm{~s}) \rightleftharpoons \mathrm{PbO}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})$$

Using data in Appendix C, calculate the equilibrium pressure of $\mathrm{CO}_2$ in the system at

$$120^{\circ} \mathrm{C}$$

Which of the following thermodynamic functions are associated only with the first law of thermodynamics : $S, U, G$, and $H$ ?

Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.

$$\ce{M3O4(s)\rightleftharpoons 3M(s) + 2O2(g)}$$

$$\begin{array}{|c|c|} \hline \text{Substance} & {\Delta G^{\circ}}_{t} \text{(kJ/mol)} \\ \hline \ce{M_{3}O_{4}} & -6.40 \\ \hline \text{M(s)} & 0 \\ \hline \ce{O}_{2}\text{(g)} & 0 \\ \hline \end{array}$$

a) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?

b) What is the equilibrium constant of this reaction, as written, in the forward direction at $\ce{298 K}$?

c) What is the equilibrium pressure of $\ce{O_{2}(g)}$ over $\ce{M(s)}$ at $\ce{298 K}$?

Write the equilibrium-constant expression and calculate the value of the equilibrium constant for each of the following reactions at $298 \mathrm{~K}$, using data from Appendix C:

$$\mathrm{NaHCO}_3(\mathrm{~s}) \rightleftharpoons \mathrm{NaOH}(\mathrm{s})+\mathrm{CO}_2(g)$$

Classify each of the following reactions as one of the four possible types summarized in Table 19.4:

$$\mathrm{N}_2 \mathrm{~F}_4(g) \longrightarrow 2 \mathrm{NF}_2(g)$$

$$\Delta H^{\circ}=85 \mathrm{~kJ} ; \Delta S^{\circ}=198 \mathrm{~J} / \mathrm{K}$$

Calculate $\Delta$S for the following reaction:

$$\ce{2PbO(s) + C(s) \longrightarrow 2Pb(s) + CO2(g)}$$

Given:

S°(PbO(s)) = 69.54 J/(K·mol)
S°(C(s)) = 5.7 J/(K·mol)
S°(Pb(s)) = 64.89 J/(K·mol)
S°(CO$_2$(g)) = 213.6 J/(K·mol)

Consider the decomposition of a metal oxide to its elements, where M represents a generic metal.

$$\ce{M2O3(s) <=> 2M(s) + \frac{3}{2}O2(g)}$$

What is the standard change in Gibbs energy for the reaction, as written, in the forward direction?

What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K?

What is the equilibrium pressure of $\ce{O2(g)}$ over $\ce{M(s)}$ at 298 K?

Consider the following reactions with the corresponding enthalpy:
A → 2B, ΔH1
A → 3C, ΔH2
What is the ΔH for reaction 2B → 3C?

a. 2 x (ΔH1 + ΔH2)

b. ΔH1 - ΔH2

c. ΔH1 + ΔH2

d. ΔH2 - ΔH1