Question

How much energy would be produced from the reaction of 2.40 moles hydrogen with 3.95 moles chlorine? ___ H2 + ___ Cl2 ___ HCl ΔH = -554 kJ

Answer 1

Answer:

How much energy would be produced from the reaction of 2.40 moles hydrogen with 3.95 moles chlorine?

$H_2 + Cl_2 -> 2HCl , deltaH = -554 kJ$

Explanation:

Given,

2.40 moles hydrogen reacts with 3.95 moles chlorine.

From the balanced chemical equation,

1mol. of H2 reacts with 1mol. of Cl2

then,

2.40mol. of H2 reacts with ----?mol of Cl2

$=>2.40 mol. H2 * \frac{1mol. Cl2}{1mol. H2} \\=2.40 mol. Cl2$

So, the remaining moles of Cl2 is in excess.

The limiting reagent is--- H2.

1mol. of H2 releases --- 554kJ of energy

then,

2.40mol of H2 releases ---- ?

$=>2.40mol * \frac{554kJ}{1 mol.} \\=1329.6kJ$

Answer is: deltaH =-1329.6kJ