1.1. At high temperatures,  gaseous phosphorus (V) chloride dissociates according to the following equation.

PCl₅ (g) ⇋ PCl₃ (g) + Cl₂ (g)

At 500K, the equilibrium amount of each gas is shown in Table 1.

Table 1

Calculate the total pressure of the reaction, if K_P = 597 kPa.

Give your answers to an appropriate number of significant figures.

1.2. Nitrogen dioxide decomposes according to the following equation.

2NO₂ (g) ⇋ 2NO (g) + O₂ (g)

At 700 K, the equilibrium amount of each gas is shown in Table 2.

Table 2

Calculate the total pressure of the reaction, if K_P = 6.8 x 10^-3 kPa.

1.3. Hydrogen iodide can undergo thermal decomposition according to the following equilibrium.

2HI (g) ⇋ H₂ (g) + I₂ (g)

The value of K_P for this reaction at 700K is 0.0185.

Calculate the total pressure when the partial pressure of hydrogen iodide, at equilibrium, is 133 kPa. Give your answer to the appropriate number of significant figures.

1.4. Dinitrogen tetroxide decomposes according to the following equilibrium.

N₂O₄ (g) ⇋ 2NO₂ (g)

The value of K_P for this reaction at 350 K is 395 kPa.

The equilibrium mixture contained 1.20 moles of nitrogen dioxide when an initial 2.00 moles of dinitrogen tetroxide were heated at 350 K.

Calculate the partial pressures of dinitrogen tetroxide and nitrogen dioxide.

Give your answer to the appropriate number of significant figures.