The reaction of hydrogen and oxygen gases produces 18.0 g of water and releases 68.2 kcal of

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The reaction of hydrogen and oxygen gases produces 18.0 g of water and releases 68.2 kcal of heat. How much energy is required to decompose 18.0 g of water into hydrogen and oxygen gases?

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The problem asks us to find the energy required to decompose 180 g of water into hydrogen and oxygenWe know the following information Reaction H2 12 O2 H2O Energy released 682 kcalmol negative sign indicates exothermic reaction Water produced 180 g 1 Find the moles of water produced Firstwe need to convert the mass of water to moles using its molar mass 180 gmol moles of water mass of water molar mass of water moles of water 180 g 180 gmol moles of water 10 mol 2 Relate energy to moles of water The energy value given 682 kcalmol represents the energy released per mole of water formedSince the decomposition reaction is the reverse of the formation reactionthe energy required to decompose 1 mole of water is equal to the negative of the energy released energy to decompose 1 mol water 682 kcalmol energy to decompose 1 mol water 682 kcalmol 3 Calculate the energy required for 180 g of water Finallywe can calculate the total energy required by multiplying the energy per mole by the number of moles of water 10 mol total energy required energy per mole moles of water total energy required 682 kcalmol 10 mol total energy required 682 kcal Therefore 682 kcal of energy is required to decompose 180 g of water into hydrogen and oxygen ...View the full answer

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