58. The reactionCaCO(s)CaQ(s) + CO:(g)is the basis of a very ancient chemical industry. Seashells or chalk (limestone) are roasted in kilns to produce CaQ.(quicklime). When moistened and used in a mortar, this forms Ca(OH): (slaked lime). Atmospheric CO₂ slowly convertsthis back to CaCO). A strong bond thus results between the stones used in the wall.Is the above reaction exothermic or endothermic? Explain.b. Lime kilns, since ancient times, have been designed with efficient chimneys to draw exhaustgases away. In terms of Le Chatslist's Principle, give two reasons why this enhances theconversion of limestone to quicklime.a.C.When a sample of CaCO,(s) is placed in a sealed, evacuated container, the equilibrium CO₂pressure at a given temperature is always the same, and is not influenced by the amount ofCaCO), provided that there is still some present at equilibrium. Explain why.d. How would the result in Part c. be affected by adding an equal number of moles of CaQ to theflask? Explain.X