Question

How many grams of Carbon would be required to react with 16g of Hydrogen gas so as to form 64g of methane gas ?​

Answer 1

Answer:

CH4 + 2 O2 → CO2 + 2 H2O

Molar mass of methane = 12+4×1 = 16 g/mol.

Molar mass of dioxygen = 2×16 = 32 g/mol.

Molar mass of carbon dioxide = 12+2×16 = 44 g/mol.

From the stoichiometric equation we get, mole ratio of methane and dioxygen = 1 : 2.

Therefore, mass ratio of methane : dioxygen = 16 : 2×32 = 16 : 64.

Given mass ratio of methane and dioxygen = 16 : 60.

It is found that, dioxygen is supplied less than required. So, dioxygen is the limiting reagent here.

Now, 64 g dioxygen produces 44 g CO2.

60 g dioxygen produces (44/64)×60 = 41.25 g.

So, the mass of resultant carbon dioxide = 41.25 g.

Mass of unreacted methane = 16 -(60/4) = 1.0 g.

Hope, this helps.