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How are forward and reverse reaction rates related in a system at chemical equilibrium?

Are ice cubes floating in \(0^{\circ} \mathrm{C}\) water in an insulated container an example of a system in dynamic equilibrium? Explain why or why not.

Do rapid reversible reactions always have greater yields of product than slow reversible reactions? Explain why or why not.

At \(1200 \mathrm{K}\) the partial pressures of an equilibrium mixture of \(\mathrm{H}_{2} \mathrm{S}, \mathrm{H}_{2},\) and \(\mathrm{S}\) are \(0.020,0.045,\) and 0.030 atm, respectively. Calculate the value of the following equilibrium constant at \(1200 \mathrm{K}\) $$ \mathrm{H}_{2} \mathrm{S}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{S}(g) \quad K_{\mathrm{p}}=? $$

Phosgene \(\left(\mathrm{COCl}_{2}\right)\) is used in the manufacture of foam rubber and bulletproof glass. It is formed from carbon monoxide and chlorine in the following reaction: $$ \mathrm{Cl}_{2}(g)+\mathrm{CO}(g) \rightleftharpoons \mathrm{COCl}_{2}(g) $$ The value of \(K_{\mathrm{c}}\) for the reaction is 5.0 at \(327^{\circ} \mathrm{C} .\) What is the value of \(K_{\mathrm{p}}\) at \(327^{\circ} \mathrm{C} ?\)

How is an equilibrium constant different from a reaction quotient?

Explain how comparing the values of reaction quotient \(Q\) and equilibrium constant \(K\) for a given reaction and temperature enables chemists to predict whether a reversible reaction will proceed in the forward direction, in the reverse direction, or in neither direction.

Mixing aqueous solutions of sodium bicarbonate and calcium chloride results in this reaction: \(2 \mathrm{NaHCO}_{3}(a q)+\mathrm{CaCl}_{2}(a q) \rightleftharpoons\) $$ 2 \mathrm{NaCl}(a q)+\mathrm{CO}_{2}(g)+\mathrm{CaCO}_{3}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell) $$ Write the \(K_{\mathrm{c}}\) expression for the reaction.

Does adding reactants to a system at equilibrium increase the value of the equilibrium constant? Why or why not?

Increasing the concentration of a reactant shifts the position of chemical equilibrium toward formation of more products. What effect does adding a reactant have on the rates of the forward and reverse reactions?