Calculation of moles of KCl required to produce 10 moles of Cl2 by the reaction with KClO3

To determine the moles of KCl required to produce 10 moles of Cl2 by the reaction with KClO3, we need to first write and balance the chemical equation for the reaction.

The balanced equation for the reaction between KClO3 and KCl to produce Cl2 can be written as follows:

2 KClO3 → 2 KCl + 3 O2

From the balanced equation, we can see that 2 moles of KClO3 react to produce 2 moles of KCl. Therefore, the molar ratio between KClO3 and KCl is 2:2, which simplifies to 1:1.

Now, we can use the concept of stoichiometry to calculate the moles of KCl required. Since the molar ratio of KClO3 to KCl is 1:1, it means that for every mole of KClO3 used, one mole of KCl is produced.

Given that we want to produce 10 moles of Cl2, which is the product of the reaction, we need to determine the moles of KClO3 required to produce this amount.

Calculation:
Moles of KClO3 required = Moles of Cl2 produced

Moles of Cl2 produced = 10 moles (given)

Therefore, Moles of KClO3 required = 10 moles

Since the molar ratio of KClO3 to KCl is 1:1, it means that 10 moles of KClO3 will produce 10 moles of KCl.

Therefore, the moles of KCl required to produce 10 moles of Cl2 is also 10 moles.

Conclusion:
The moles of KCl required to produce 10 moles of Cl2 by the reaction with KClO3 is 10 moles. This is based on the balanced chemical equation and the stoichiometry of the reaction, where the molar ratio between KClO3 and KCl is 1:1.