Question

What coefficient would you place in front of O2 in order to balance this chemical equation:

2C2H6 + _?_O2 → 4CO2 + 6H2O

C)8 A) 6 R) 14 B) 7

Answer 1

7 O2

Step-by-step explanation:

You are given the balanced equation 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(ℓ) You are given rules for assigning oxidation numbers in Table 9.3 on page 604 of the student textbook. Compare the oxidation numbers of the atoms of each element on both sides of the equation. ... Therefore, the reaction is a redox reaction.

Answer 2

7 O2

Step-by-step explanation:

My method involves counting all the elements in the equation. There must be an equal amount of each on both sides. Because it's asking for O2 only, look for compounds that deal with O2

So...CO2 and H2O only on the product side for this chemical equation.

Count the total O there is

CO2 has 2 O in one molecule, so 4 CO2 molecule is 8 Oxygen

H2O has 1 O in one molecule, so 6 H2O molecule is 6 Oxygen.

Your total O on the product side is 14

On the reactant side, the O2 is paired because O2 likes to be stable, so one O2 molecule has 2 O. This means that 2x = 14, which is 7.

Your answer is 7