Problem: In the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as auto headlamps, acetylene is still used as a source of light by some cave explorers. The acetylene is (was) prepared in the lamp by the reaction of water with calcium carbide, CaC2: CaC2(s) + 2H2O(l) ⟶ Ca(OH)2(s) + C2H2(g)Calculate the standard enthalpy of the reaction. The ΔH°f of CaC2 is −15.14 kcal/mol.

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FREE Expert Solution

ΔH°rxn=ΔH°f, prod-ΔH°f, react


Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol. 


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Problem Details

In the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as auto headlamps, acetylene is still used as a source of light by some cave explorers. The acetylene is (was) prepared in the lamp by the reaction of water with calcium carbide, CaC2

CaC2(s) + 2H2O(l) ⟶ Ca(OH)2(s) + C2H2(g)

Calculate the standard enthalpy of the reaction. The ΔH°f of CaC2 is −15.14 kcal/mol.

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Based on our data, we think this problem is relevant for Professor Blankenship's class at UGA.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.