A sample of 1.6 g of methane (CH4) is completely burnt in 20.00 g of oxygen. The products are carbon dioxide and water. Which is the excess reactant? Which is the limiting reactant? How much of the excess reactant remains unreacted?

Question

Chemistry

Ronnie Hale

11 July, 02:30

A sample of 1.6 g of methane (CH4) is completely burnt in 20.00 g of oxygen. The products are carbon dioxide and water. Which is the excess reactant? Which is the limiting reactant? How much of the excess reactant remains unreacted?

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Answers (1)

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Larry · Answer 1

Equation of reaction:

CH₄ + 2O₂ → CO₂ + 2H₂O CH₄ = 16g/mole O₂ = 32g/mole

16 2*32

16g of CH₄ would react completely with 64g Oxygen gas.

Therefore

1.6g of CH₄ would require 6.4g Oxygen gas (Divide through by 10)

But from question:

1.6g of CH₄ was burnt completely in 20g of Oxygen gas.

a). We can see that the oxygen reactant was in excess as only 6.4g would take part in the reaction.

b). The limiting reactant is the Methane CH₄, it is the one that is less available.

c.) Excess reactant is Oxygen. Excess by = 20 - 6.4 = 13.6g