# 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)?

Mar 29, 2018

Approx. $450 \cdot k c a l$...

#### Explanation:

You gots...

$2 C {l}_{2} \left(g\right) + 7 {O}_{2} \left(g\right) + 130 \cdot k c a l \rightarrow 2 C {l}_{2} {O}_{7} \left(g\right)$

Another way of writing this is as...

$2 C {l}_{2} \left(g\right) + 7 {O}_{2} \left(g\right) \rightarrow 2 C {l}_{2} {O}_{7} \left(g\right)$ $\Delta {H}_{\text{rxn}}^{\circ} = + 130 \cdot k c a l \cdot m o {l}^{-} 1$

And when we write $m o {l}^{-} 1$ we mean per mole of reaction as written...and so to get $7 \cdot m o l$ of the the product...we need $\frac{7}{2}$ moles of reaction as written, with the associated enthalpy change....