a mixture of 0.5 mol H2(g) and 0.5 mol 02(g) is allowed to react in a container of volume 200 cm3 .represent in the table

To represent the reaction of a mixture of 0.5 mol H2(g) and 0.5 mol O2(g) in a container of volume 200 cm3, you can use a balanced chemical equation. The balanced equation for the reaction of hydrogen gas (H2) and oxygen gas (O2) to form water vapor (H2O) is:

2H2(g) + O2(g) -> 2H2O(g)

Here's how you can represent this reaction in a table format:

Reactants | Coefficients | Products
-------------------------------------------
H2(g) | 0.5 mol | 2H2O(g)
O2(g) | 0.5 mol |

In the reactants column, you write the chemical formula and the number of moles for each reactant. In this case, the reactants are H2(g) and O2(g), and both have 0.5 mol. The reactants don't have any coefficients because their stoichiometric ratio is 1:1.

In the products column, you write the chemical formula and the number of moles for each product. In this case, the product is 2H2O(g) since the balanced equation shows that 2 moles of water are formed for every 1 mole of hydrogen and 1 mole of oxygen reacted.

Note: The volume of the container (200 cm3) is not directly represented in the table as it is not relevant to the stoichiometry of the reaction.