What is the enthalpy change ($\Delta$H) in kJ for the following reaction?

2Al(s) + Fe$_2$O$_3$(s) $\longrightarrow$ 2Fe(s) + Al$_2$O$_3$(s)

Use the enthalpy changes for the combustion of aluminum and iron:

2Al(s) + $\frac{3}{2}$O$_2$(g) $\longrightarrow$ Al$_2$O$_3$(s) $\,\,\,\,\,\,\,\,\,\,\,\,\Delta$H = -1676.0 kJ

2Fe(s) + $\frac{3}{2}$O$_2$(g) $\longrightarrow$ Fe$_2$O$_3$(s) $\,\,\,\,\,\,\,\,\,\,\,\,\Delta$H = -822.1 kJ

Calculate ΔHrxn for the following reaction:

Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

Use the following reactions and given ΔH′s.

2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ

CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ

Classify the following chemical reaction

$$\ce{ CaCO3(s) \longrightarrow CaO(s) + CO2(g)}$$

The heat capacity of a calorimeter plus 200 mL of water is 1170 J/K. When 100.0 mL of 0.500 M HCl were mixed with 100.0 mL of 0.500 M NaOH into that coffee-cup calorimeter, the temperature went from 22.5°C to 24.9°C. Calculate ΔH for the process.

In a coffee cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl are mixed. Both solutions were orignially at $24.6 ^ { \circ } \mathrm { C }.$ After the reaction, the final temperature is $31.3 ^ { \circ } \mathrm { C }.$ Assuming that all the solutions have a density of $1.0\ \mathrm { g } / \mathrm { cm } ^ { 3 }$ and a specific heat capacity of $4.18\ \mathrm { J } ^ { \circ } \mathrm { C } ^ { -1 } \mathrm { g } ^ { - 1 } ,$ calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

Compare your answers with those at the back of the book.

The chm is another name for which of the following? (8.2)

(a) wolt per ampere

(b) ampere per wolt

(c) watt

(d) volt

From the following data,

$$\begin{aligned} & \mathrm{C} \text { (graphite) }+\mathrm{O}_2(g) \mathrm{CO}(g) \\ & \Delta H_{\mathrm{rxn}}^{\circ}=-393.5 \mathrm{~kJ} / \mathrm{mol} \\ & \mathrm{H}_2(g)+\frac{1}{2} \mathrm{O}_2(g) \longrightarrow \mathrm{H}_2 \mathrm{O}(l) \\ & \Delta H_{\mathrm{rxn}}^{\circ}=-285.8 \mathrm{~kJ} / \mathrm{mol} \\ & 2 \mathrm{C}_2 \mathrm{H}_6(g)+7 \mathrm{O}_2(g) \longrightarrow 4 \mathrm{CO}_2(g)+6 \mathrm{H}_2 \mathrm{O}(l) \\ & \Delta H_{\mathrm{rxn}}^{\circ}=-3119.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned}$$

calculate the enthalpy change for the reaction

$$2 \mathrm{C} \text { (graphite })+3 \mathrm{H}_2(g) \longrightarrow \mathrm{C}_2 \mathrm{H}_6(g)$$

Carbon reacts with oxygen to produce carbon dioxide $\ce{(CO2 (g), \Delta Hf = –393.5 kJ/mol)}$ according to the equation below:

$$\ce{C(s) + O2(g) -> CO2(g)}$$

What is the enthalpy change of the reaction?

A) $\ce{-393.5 kJ}$
B) $\ce{-196.8 kJ}$
C) $\ce{196.8 kJ}$
D) $\ce{393.5 kJ}$

Using the following data, calculate $\Delta H_{f}°$ for CO(g):

$$\begin{align*} \mathrm{C}(graphite)+\mathrm{O_2}(g)&\rightarrow\mathrm{CO_2}(g)\;\;\;\;\;\;\Delta H_{rxn}°=-393.5\;\mathrm{kJ/mol}\\ \mathrm{CO}(g)+\dfrac{1}{2}\;\mathrm{O_2}(g)&\rightarrow\mathrm{CO_2}(g)\;\;\;\;\;\;\Delta H_{rxn}°=-283.0\;\mathrm{kJ/mol} \end{align*}$$

(a) -393.5 kJ/mol (b) -676.5 kJ/mol (c) +676.5 kJ/mol (d) +110.5 kJ/mol (e) -110.5 kJ/mol

A 0.1375-g sample of solid magnesium is burned in a constant-volume bomb calorimeter that has a heat capacity of 3024 J/°C. The temperature increases by 1.126 °C. Calculate the heat given off by the burning Mg, in kJ/g and in kJ/mol.

A piece of silver with a mass of 362 g has a heat capacity of 85.7 J/°C. What is the specific heat of silver?

Calculate the heat of formation for ethane from the following:

$$\ce{ C2H6 (g) \rightarrow 2C (s) + 3H2 (g); \Delta H = 31 kJ mol^{-1}}$$

Calculate the standard enthalpy change for this reaction, using heat of formation.

Calculate the standard enthalpy change of the methanol combustion reaction.