How many moles of oxygen will be produced from the decomposition of 3 moles of #KClO_3# in the reaction #KClO_3 -> KCl + O_2#?

Answer 1

Mateo Aguilar

We first have to balance the equation, because it isn't.

#KClO_3>KCl+1 1/2 O_2# because there are three #O#'s

Or rather: #2KClO_3->2KCl+3 O_2#

This doesn't matter for the solution because every mole of #KClO_3# will produce #1 1/2# mole of #O_2#

The final portion is doable.

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Answer 2

Henry Antrim

According to the balanced chemical equation, 2 moles of KClO3 produce 3 moles of O2. Therefore, if 3 moles of KClO3 decompose, it will produce (3 , \text{moles} \times \frac{3 , \text{moles O}_2}{2 , \text{moles KClO}_3} = 4.5 , \text{moles O}_2.)

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

How many moles of oxygen will be produced from the decomposition of 3 moles of #KClO_3# in the reaction #KClO_3 -&gt; KCl + O_2#?

How many moles of oxygen will be produced from the decomposition of 3 moles of #KClO_3# in the reaction #KClO_3 -> KCl + O_2#?