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How do you calculate the energy required to produce 7.00 mol $Cl_2O_7$ on the basis of the following balanced equation: $2Cl_2(g) + 7O_2(g) + 130 kcal -> 2Cl_2O_7(g)$?

Md Ariful Islam

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Md Ariful Islam

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$2Cl_2(g) + 7O_2(g) + 130*kcal rarr 2Cl_2O_7(g)$

Another way of writing this is as...

$2Cl_2(g) + 7O_2(g) rarr 2Cl_2O_7(g)$ $DeltaH_"rxn"^@=+130*kcal*mol^-1$

And when we write $mol^-1$ we mean per mole of reaction as written...and so to get $7*mol$ of the the product...we need $7/2$ moles of reaction as written, with the associated change....

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