Question

For the balanced reaction below, determine the limiting reactant if 1.5 moles of methane reactswith 2.0 moles of oxygen. Show all your workCH4(8) + 2O2(g) → CO2(g) + 2H2O(g)(methane)

Answer 1

Oxygen is the limiting reactant in the reaction

Step-by-step explanation

Given information

`\text{ CH}_(4(g))+\text{ 2O}_(2(g))\rightarrow\text{ CO}_(2(g))\text{ + 2H}_2O(g)`

The mole of methane is 1.5 moles

The mole of oxygen is 2.0 moles

To determine the limiting reactant in the reaction above, follow the steps below

Step 1: Write the formula for calculating the limiting reactant in a reaction

`\text{ = }\frac{moles}{stoichiometric\text{ coefficient of the reactant}}`

Step 2: write the stoichiometric coefficient of the reactants in the above equation

The stoichiometric coefficient of methane is 1

The stoichiometric coefficient of oxygen is 2

Step 3: Divide the mole of the reactants by their stoichiometric coefficient

`\begin{gathered} \text{ Methane = }(1.5)/(1) \\ \text{ Methane = 1.5 mol/wt } \\ \\ \text{ Oxygen = }(2.0)/(2) \\ \text{ oxygen = 1 mol/wt} \end{gathered}`

From the above calculations, you will see that oxygen has the least mole per weight.

Therefore, oxygen is the limiting reactant in the above reaction