Consider the combustion of methanol at some high temperature in a constant-pressure reaction chamber: 2ch3oh (g) + 3o2 (g) \longrightarrow ⟶ 2co2 (g) + 4h2o (g) if you react 10 l of oxygen gas with 18 l of methanol gas, what will the final volume be?

Answer : The final volume of the reaction mixture is 31.33 L

Explanation :

The given balanced chemical equation is ,

Step 1 : Find limiting reactant

In order to find the limiting reactant, we will divide the given volumes by the stoichiometric coefficient from the balanced equation. The reactant that gives lower volume is the limiting reactant.

Since the volume of O₂ is lower, it is the limiting reactant.

Step 2 : Using limiting reactant, find out the volumes of product formed.

The amount of CO₂ formed can be calculated as,

The amount of H₂O formed can be calculated as,

Total volume of products = 6.67 L + 13.33 L = 20 L

Step 3 : Find the volume of excess reactant.

The amount of methanol that reacts with the given amount of O₂ is

But the initial amount of methanol is 18 L.

The amount of excess reactant is 18 L - 6.67 L = 11.33 L

The total volume of gases after the reactant is complete = total volume of products + excess reactant = 20 L + 11.33 L = 31.33 L

The final volume of the reaction mixture is 31.33 L

b.

the accuracy of the data.

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8