The Haber process is the principal industrial route for converting nitrogen into ammonia:

$$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_3(\mathrm{~g})$$

Using the thermodynamic data in Appendix C, calculate the equilibrium constant for the process at room temperature.

The molar solubility of PbI2 is 1.5 x 10-3 M.

a) What is the molar concentration of iodide ion in a saturated PbI2 solution?

b) Determine the solubility constant, Ksp, for lead(II) iodide.

Calculate the solubility of each of the following compounds in mole/L. Ignore any acid-base properties:

$\ce{Hg2Cl2}$. $K_\ce{sp}$= $\pu{1.1 x10^-18}$ ($\ce{Hg2^2+}$ is the cation in the solution. )

Calculate the energy carried by $1.40$ moles of infrared photons whose wavelength is $814\ \text{nm}$.

A system releases 605kJ of heat and does 100 kJ of work on the surroundings. What is the change in internal energy of the system?

What is the change in the internal energy of the system?

The blood alcohol concentration (BAC) of a person who has been drinking is approximated by the following formula. $\mathrm{BAC}=$ number of $\mathrm{oz} \times \%$ alcohol $\times 0.075 \div$ body wt in $\mathrm{lb}-\mathrm{hr}$ of drinking $\times 0.015$. Calculate the BAC to the nearest thousandth for a 135-lb woman who, in 3 hr, has consumed three 12-oz beers (36 oz), each having a 4.0% alcohol content.

A 1967 Kennedy half-dollar has a mass that is

$$1.150 \times 10 ^ { - 2 } \mathrm { kg }$$

The coin is a mixture of silver and copper, and in water weighs 0.1011 N. Determine the mass of silver in the coin.

The work function of palladium is $5.22 \mathrm{eV}$. What is the minimum frequency of light required to observe the photoelectric effect on $\mathrm{Pd}$ ? If light with a $200 . \mathrm{nm}$ wavelength is absorbed by the surface, what is the velocity of the emitted electrons?

Dinitrogen tetroxide decomposes to nitrogen dioxide: $\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \quad \Delta H_{\mathrm{rxn}}^{\mathrm{o}}=55.3 \mathrm{kJ}$ At 298 K, a reaction vessel initially contains 0.100 atm of $N_2O_4$. When equilibr ium is reached, 58% of the $N_2O_4$ has decomposed to $NO_2$. What percentage of $N_2O_4$ decomposes at 388 K? Assume that the initial pressure of $N_2O_4$ is the same (0.100 atm) .

Calculate the final pressure of a sample of carbon dioxide that expands reversibly and adiabatically from 57.4 kPa and 1.0 dm$^3$ to a final volume of 2.0 dm$^3$. Take ? = 1.4.

Calculate the final pressure of a sample of water vapour that expands reversibly and adiabatically from 87.3 Torr and 500 cm$^3$ to a final volume of 3.0 dm$^3$. Take ? = 1.3.

The drawing on the left represents a buffer composed of equal concentrations of a weak acid, $\mathrm{HX}$, and its conjugate base, $X^{-}$. The heights of the columns are proportional to the concentrations of the components of the buffer.

Which of the three drawings (1), (2), (3) represents the buffer after the addition of a strong acid?

The drawing on the left represents a buffer composed of equal concentrations of a weak acid, $\mathrm{HX}$, and its conjugate base, $X^{-}$. The heights of the columns are proportional to the concentrations of the components of the buffer.

Which of the three represents a situation that cannot arise from the addition of either an acid or a base?

The drawing on the left represents a buffer composed of equal concentrations of a weak acid, $\mathrm{HX}$, and its conjugate base, $X^{-}$. The heights of the columns are proportional to the concentrations of the components of the buffer.

Which of the three represents the buffer after the addition of a strong base?