Calcium oxide and water react in an exothermic reaction: CaO(s) + H₂O(l) $\rarr$ Ca(OH)₂(s), $\Delta$H^$\circ$_rxn = -64.8 kJ/mol.How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152g H₂O A) 1.97 * 10^-3 kJ B) 8.26 kJ C) 508 kJ D) 547 kJ E) 555 kJ

Question

Quizplus · Accepted Answer

The reaction of calcium oxide (CaO) with water is exothermic, releasing -64.8 kJ/mol of heat. To find the heat released by 7.15 g of CaO, first, calculate the moles of CaO (molar mass of CaO ≈ 56.08 g/mol). Moles of CaO = 7.15 g / 56.08 g/mol ≈ 0.1275 mol. Then, multiply the moles by the heat released per mole: 0.1275 mol * -64.8 kJ/mol ≈ -8.26 kJ.

Calcium Oxide and Water React in an Exothermic Reaction: CaO(s) →\rarr→

Calcium Oxide and Water React in an Exothermic Reaction: CaO(s) $\rarr$