In the decomposition of KCLO3 how many mole of KCL are formed in the reaction that produce 0.05 mole of O2

Answer 1

The balanced equation for the decomposition of KCLO3 is:

2KCLO3(s) → 2KCl(s) + 3O2(g)

From the equation, we can see that 2 moles of KCLO3 produce 2 moles of KCl. Therefore, to determine how many moles of KCl are formed when 0.05 moles of O2 are produced, we need to first calculate how many moles of KCLO3 are required to produce 0.05 moles of O2.

Using the mole ratio from the balanced equation, we know that 2 moles of KCLO3 produce 3 moles of O2. Therefore, to produce 0.05 moles of O2, we need:

0.05 moles O2 × (2 moles KCLO3 / 3 moles O2) = 0.0333 moles KCLO3

Now that we know we need 0.0333 moles of KCLO3 to produce 0.05 moles of O2, we can use the mole ratio from the balanced equation to determine how many moles of KCl are produced:

0.0333 moles KCLO3 × (2 moles KCl / 2 moles KCLO3) = 0.0333 moles KCl

Therefore, 0.0333 moles of KCl are formed in the reaction that produces 0.05 mole of O2.

Answer 2

2KClO3 → 2KCl + 3O2
so 2/3 * 1/20 = 1/30 mole of KCl