Determine the enthalpy for this reaction:

Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l)
Substance ΔHf∘ (kJ/mol)

CO2(g) −393.5

Ca(OH)2(s) −986.1

H2O(l) −285.8

CaCO3(s) −1207.0

H2O(g) −241.8

The Enthalpy for the reaction will be -113.2 kJ/mol

Explanation:

→

We know that, Ideal Enthalpy of formation = ( Net Enthalpy of the products) -( Net Enthalpy of reactants) at 298K temperature.

So, Δ = ( Δ +Δ) - (Δ + Δ)

            = (- 1207.0 - 285.8) - ( -986.1 - 393.5)

           = -1492.8 +1379.6

          = -113.2 kJ/mol

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.