In an aqueous solution of sodium carbonate (Na_2CO_3), the following equilibrium

Question

In an aqueous solution of sodium carbonate (Na_2CO_3), the following equilibrium occurs: CO_3^2-(aq) + H_2O(l) HCO_3^-(aq) + OH^-(aq) How would the addition of solid sodium hydrogen carbonate (NaHCO_3) affect this equilibrium mixture? Briefly explain. If a small volume of HCI solution were added, how would the equilibrium change? Briefly explain. Carbon monoxide (CO) and hydrogen (H_2) gases are produced when water vapor is passed over carbon (graphite). C(s) + H_2O(g) CO(g) + H_2(g) The forward reaction is endothermic. If the equilibrium mixture is heated, how will the equilibrium be affected? Briefly explain. When a saturated solution of sodium nitrate (NaNO_3) is prepared, the following equilibrium exists: NaNO_3(s) Na^+(aq) + NO_3^-(aq) If HNO_3 is added to the saturated solution, what change will be observed? Briefly explain. The dissolution of NaNO_3 is endothermic. What change in reaction conditions would cause more NaNO_3(s) to dissolve? Briefly explain. One step in the production of H_2SO_4 involves the equilibrium: 2SO_2(g) +O_2(g) 2SO_3(g) The reaction is exothermic. At equilibrium, only about 80% of the SO_2 is converted to SO_3. Suggest two ways in which the equilibrium yield of SO_3 might be increased.

Explanation / Answer

1. By the addition of NaHCO3, the concentration of HCO3 increase, by Le Chatelier principle to compensate this chage the equilibrium shifts to the opposite side of the concentration increase, therefore, the equilibrium shifts to the left.

2. by the addition of H+, the OH in the right is neutralized so its concentration decreases, to compensate this fact the equilibrium shifts to the right. (side of the decreased concentration)

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