Question

A reaction involves the following elementary steps:

H2​(g)+O2​(g) ------> H2​O2​(g)

H2​(g)+H2​O2​(g) ------>2H2​O(g)

a)What is the sum of the two reactions, retaining all chemical species? Remember to include states of matter.

b)What is the net reaction when reactive intermediates are cancelled? Please include states of matter.

Answer 1

Step-by-step explanation:

H₂
`_(g)` + O₂
`_(g)` → H₂O₂
`_(g)`

H₂
`_(g)` + H₂O₂
`_(g)` → 2H₂O
`_(g)`

The sum of the two equations is a combined equation where all the compounds on the reactant sides are written on the Left hand side and the products are all on the right hand side:

• H₂
  `_(g)` + O₂
  `_(g)` + H₂
  `_(g)` + H₂O₂
  `_(g)` → H₂O₂
  `_(g)` + 2H₂O
  `_(g)`

• The net reaction equation involves the cancellation of species that occurs on both sides, these species are H₂O₂:

We then have:

H₂
`_(g)` + H₂
`_(g)` + O₂
`_(g)` → 2H₂O
`_(g)`

combining the two repeating hydrogen gas:

2H₂
`_(g)` + O₂
`_(g)` → 2H₂O
`_(g)`