Question

<p>1. The equilibrium of ice and water at 0^oC and 1 atm pressure can be expressed by the chemical equation:<br /><br />Ice(s)--&gt;&lt;--water(l)<br /><br />a) is the forward reaction exothermic or endothermic?<br /><br />b) Using Le Chatelier's Principle, explain why liquid water spontaneously converts to solid ice when the temperature drops below 0^oC (at 1 atm).<br /><br />c) From your own experience, state if a given amount of H2O occupies a larger volume in the form of solid ice or of liquid water. (HINT&gt; does ice float or sink?)<br /><br />d) Using Le Chatelier's Principle, explain what happens to the ice/water equilibrium when pressure is raised to 2 atm (at 0^oC)<br /><br /><br /><br />2. Hydrated ionic compounds such as CuSO4 x 5H2O and CaSO4 x 2H2O (gypsum) spontaneously convert to their anhydrous forms (CuSO4 and CaSO4, respectively) as the temperature is raised.<br /><br />a) For each of these two compound, write a balanced chemical equation expressing the equilibrium between the hydrated and anhydrous form.<br /><br />b) Use Le Chatelier's Principle to predict if the change of the anhydrous to the hydrated compounds is expected to be accompanied by the absorption or by release of heat. explain you conclusion.</p>