An atomic hydrogen torch is used for cutting and welding thick sheets of metal. When H₂ passes through an electric arc, the molecules decompose into atoms, which react with O₂. Temperatures over 5000°C are reached, which can melt all metals. Write equations for the breakdown of H₂ to H atoms and for the subsequent overall reaction of the H atoms with oxygen. Use Appendix B to find the standard enthalpy of each reaction per mole of product.

Question

contestada

Respuesta :

tanisharawat014 tanisharawat014 · Answer 1 · 2022-08-31T04:12:51+02:00

The Delta H or standard enthalpy of reaction is -677.826kj/mol .

Given,

An atomic hydrogen torch is used to cutting and welding thick sheets of metal.

When H2 passes through an electric arc, the molecules decomposes in to atoms, which react with O2.

Temperatures over 5000°C are reached, which can melt all metals.

The equation of the breakdown of H2 to H atoms is given by,

H2(g) +heat ------> 2H(g)

The equation for the H atoms with oxygen is given by,

4H(g) + O2(g) ----------->2H2O(g)

The product also remains in gaseous state as the temperature is very high.

Now,

Delta H rxn =Delta H products - delta H reactants

=2(-241.826KJ/mol) - (4×218.0 KJ/mol)

=-1355.652Kj/mol

This is the Delta H for 2 moles of product.

Thus, Delta H for 1 mol of product = -1355.652/2

= -677.826Kj/mol

Hence, the Delta H or enthalpy of reaction per mole of product is 677.826kj/mol .

Learn more about enthalpy here :

brainly.com/question/14291557

#SPJ4