Study the scenario and the balanced equation.

While a Bunsen burner is ignited, 7.45 x 1024 mol of methane (CH4) reacts with an excess of oxygen (O2).

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g)

(M H2O = 18.0 g/mol; M CH4 = 16.0 g/mol)

What is the theoretical yield of water produced?

A) 2.68 * 1026 mol H2O

B) 4.14 * 1023 g H2O

C) 4.14 * 1023 mol H2O

D) 2.68 * 1026 g H2O

Option-D (2.68 * 10²⁶ g of H₂O)

Explanation:

The balance chemical equation for the combustion of Methane is as follow;

CH₄ + 2 O₂ → CO₂ + 2 H₂O

According to balanced equation,

1 mole of CH₄ produced = 2 moles of H₂O

So,

7.45 * 10²⁴ moles of CH₄ will produce = X moles of H₂O

Solving for X,

X = 7.45 * 10²⁴ mol * 2 mol / 1 mol

X = 1.49 * 10²⁵ mol of H₂O

As there is no option containing calculated moles of H₂O produced so, we will convert the moles of H₂O to mass and then look for that answer in given choices.

As,

Mass = Moles * M. Mass

Mass = 1.49 * 10²⁵ mol * 18.01 g/mol

Mass = 2.68 * 10²⁶ g of H₂O

Okay! That's Option-D.