How many moles of hydrogen are needed to produce 13.78 mol of ethane?

This is an incomplete question, here is a complete question.

The following balanced equation shows the formation of ethane (C₂H₆).

How many moles of hydrogen are needed to produce 13.78 mol of ethane?

1) 3.445 mol

2) 6.890 mol

3) 27.56 mol

4) 55.12 mol

Answer : The number of moles of hydrogen needed are, (3) 27.56 mol

Explanation : Given,

Moles of ethane = 13.78 mol

The given balanced chemical reaction is:

From the balanced chemical reaction we conclude that,

As, 1 mole of ethane produced from 2 moles of hydrogen

So, 13.78 mole of ethane produced from moles of hydrogen

Thus, the number of moles of hydrogen needed are, 27.56 mol

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: