Question

2 c2h2(g) 5 o2(g) 4 co2(g) 2 h2o(g) how many grams fo o2(g) are needed to completely combust 13.02 g of c2h2(g)?

Answer 1

The amount of O₂(g) needed to completely combust 13.02 grams of C₂H₂(g) is 6.4 grams.

The provided chemical is,

2C₂H₂(g) + 5O₂(g) → 4CO₂(g) + 2H₂O(g)

So, from the above equation, we can see,

2 moles of C₂H₂ requires 5 moles of O₂ to completely combust.

So, we can write,

2 Moles C₂H₂ = 5 Moles O₂

Moles = Given mass/Molar mass

Given mass of C₂H₂ = 13.02 g

Molar mass of C₂H₂ = 26g/mol

Molar mass of O₂ = 32 g/mol

So. putting value,

2 x 13.02/26  = 5 x Required mass of O₂/32

Required mass of O₂ = 6.4 grams.

So, a total of 6.4 grams of Oxygen is required to completely combust 13.02 g of C₂H₂(g).

To know more about Moles, visit,

https://brainly.com/question/15356425

#SPJ4