Consider the gas-phase reaction 2 CO (g) + O2 (g) <=> 2 CO2 (g) Predict the shift in the equilibrium position when helium gas is added to the equilibrium mixture (a) at constant pressure and (b) at constant volume.

Water is a very weak electrolyte that undergoes the following ionization (called autoionization) H2O (l) <=> H^+ (aq) + OH^- (aq) (a) If k_1 = 2.410^-5 s^-1 and k_(-1) = 1.310^11 /M s, calculate the equilibrium constant K where K= [H1][OH2]/[H2O]. (b) Calculate the product [H^+][OH^-] and [H^+] and [OH^-].

The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63*10^-3 at 527 degree C: COCl2 (g) <=> CO (g) + Cl2 (g) Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm.

Consider the following equilibrium systems: (a) A <=> 2 B ; $\Delta H^\circ$ = 20.0 kJ/mol (b) A + B <=> C ; $\Delta H^\circ$ = -5.4 kJ/mol (c) A <=> B ; $\Delta H^\circ$ = 0.0 kJ/mol Predict the change in the equilibrium constant Kc that would occur in each case if the temperature of the reacting system were raised.

Explain the effect of each of the following stresses on the position of the following equilibrium:

$$3 NO(g) ↔N2O(g) + NO2(g)$$

The reaction as written is exothermic. (a) N2O(g) is added to the equilibrium mixture without change of volume or temperature. (b) The volume of the equilibrium mixture is reduced at constant temperature. (c) The equilibrium mixture is cooled. (d) Gaseous argon (which does not react) is added to the equilibrium mixture while both the total gas pressure and the temperature are kept constant. (e) Gaseous argon is added to the equilibrium mixture without changing the volume.

Consider the following reaction at a certain temperature A2 + B2 <=> 2 AB The mixing of 1 mole of A2 with 3 moles of B2 gives rise to x mole of AB at equilibrium. The addition of 2 more moles of A2 produces another x mole of AB. What is the equilibrium constant for the reaction?

For the reaction

$$\mathrm{N}_2(g)+\mathrm{O}_2(g) \rightleftharpoons 2 \mathrm{NO}(g)$$

the equilibrium constant $K$ has the value $1.71 \times 10^{-3}$ at a particular temperature. If the concentrations of both $\mathrm{N}_2(g)$ and $\mathrm{O}_2(g)$ are $0.0342 \mathrm{M}$ in an equilibrium mixture at this temperature, what is the concentration of $\mathrm{NO}(g)$ under these conditions?

For the reaction H2 (g) + CO2 (g) <=> H2O (g) + CO (g) at 700 degree C, Kc 5 0.534. Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.300 mole of CO and 0.300 mole of H2O is heated to 700°C in a 10.0-L container.

Consider the reaction 2 NO (g) + O2 <=> 2 NO2 At 430 degree C, an equilibrium mixture consists of 0.020 mole of O2, 0.040 mole of NO, and 0.96 mole of NO2. Calculate Kp for the reaction, given that the total pressure is 0.20 atm.

The equilibrium constant KP for the reaction 2SO2(g) + O2(g) <=> 2SO3(g) is 5.60*10^4 at 350 degree C. The initial pressures of SO2 and O2 in a mixture are 0.350 atm and 0.762 atm, respectively, at 350 degree C. When the mixture equilibrates, is the total pressure less than or greater than the sum of the initial pressures (1.112 atm)?

From the Arrhenius equation, predict how, a. increasing the experimental activation energy affects the rate constant for a reaction. b. increasing the temperature affects the rate constant for a reaction.

The vapor pressure of mercury is 0.0020 mmHg at 26 degree C. (a) Calculate Kc and Kp for the process Hg(l) <=> Hg(g). (b) A chemist breaks a thermometer and spills mercury onto the floor of a laboratory measuring 6.1 m long, 5.3 m wide, and 3.1 m high. Calculate the mass of mercury (in grams) vaporized at equilibrium and the concentration of mercury vapor in mg/m3. Does this concentration exceed the safety limit of 0.05 mg/m3? (Ignore the volume of furniture and other objects in the laboratory.)

Consider the following equilibrium reaction in a closed container: CaCO3 (s) <=> CaO (s) + CO2 (g) What will happen if (a) the volume is increased; (b) some CaO is added to the mixture; (c) some CaCO3 is removed; (d) some CO2 is added to the mixture; (e) a few drops of a NaOH solution are added to the mixture; (f ) a few drops of a HCl solution are added to the mixture (ignore the reaction between CO2 and water); (g) temperature is increased?

Determine the initial and equilibrium concentrations of HI if the initial concentrations of H2 and I2 are both 0.16 M and their equilibrium concentrations are both 0.072 M at 430 degree C. The equilibrium constant (Kc) for the reaction H2(g) + I2(g) <=> 2HI(g) is 54.2 at 430 degree C.