Answer:
<em>17.94 kg of water</em>
Explanation:
The combustion reaction of balanced butane (C₄H₁₀) is as follows:
2 C₄H₁₀ + 13 O₂ ⇒ 8 CO₂ + 10 H₂O
The amount of butane molecules can be transferred to moles to establish the stoichiometric relationship with water and calculate the moles of water that are formed:
6.02x10²³ molecules _____ 1 mol of butane
1.2x10²⁶ molecules _____ X = 199.34 moles of butane
<em>Calculation</em>: 1.2x10²⁶ molecules x 1 mol / 6.02x10²³ molecules = 199.34 moles of butane
According to the balanced equation:
2 moles butane _____ 10 moles of water
199.34 moles of butane _____ X = 996.68 moles of water
<em>Calculation</em>: 199.34 moles x 10 moles / 2 moles = 996.68 moles of water
And now, you can calculate the mass of the amount of moles obtained from water:
1 mole of water _____ 18 g
996.68 moles of water _____ X = <em>17.94 kg of water
</em>
<em>Calculation</em>: 996.68 moles x 18g / 1 mole = 17940.20g ≡ 17.94 kg of water
Therefore, <em>the combustion of 1.2x10²⁶ butane molecules produces 17.94 kg of water</em>.
