4537 Shares

Topic: **How to write a decomposition reaction****Question:**
Hi everyone! Okay, so here's the problem:
The decomposition of potassium chlorate, KCLO3, is used as a source of oxygen in the laboratory. How many moles of potassium chlorate are needed to produce 15 mol of oxygen gas?
Alright, so first off, I wrote the mole ratios:
KClO3 -> K + ClO + O2
I think that ratio was wrong, but the textbook did not deal with any reactions like this, since it doesn't really give you the equation? I just thought O2 is oxygen gas...
so the ratio is 1 mol KClO3 / 1 mol O2
Then, I put it in the equation, with variable x as the amount of moles of potassium chlorate needed to produce 15 mol of oxygen gas.
x mol KClO3 x 1 mol O2/ 1 mol KClO3 = 15 mol O2
Then, I got 15 mol O2, and I'm pretty sure that is wrong, since the answer key says the correct answer is 10. Anyways, I think there's something I did wrong in writing the equation and finding the ratios (wrong ratio, I suppose, but I don't know why or what I did)
Help would be very much appreciated!

June 16, 2019 / By Krista

Actually I don't like to write an extra answer to the questions already answered, if I don't see any point to be corrected. The decomposition reaction is wrong. Potassium is one of the most active elements and it cannot be obtained by heating one of its salt. Even in pure form, it is stored in gasoline because it is easily oxidized by the oxygen in air. Any way, the correct decomposition reaction; 2KClO3 (s) ----------> 2KCl (s) + 3O2 (g) For 3 moles of O2, we need 2 moles of KClO3 For 15 moles of O2, we need; 2 mol KClO3 x (15 mol O2 / 3 mol O2) = 10 mol KClO3

👍 150 | 👎 1

Did you like the answer? We found more questions related to the topic: **How to write a decomposition reaction**

Actually I don't like to write an extra answer to the questions already answered, if I don't see any point to be corrected. The decomposition reaction is wrong. Potassium is one of the most active elements and it cannot be obtained by heating one of its salt. Even in pure form, it is stored in gasoline because it is easily oxidized by the oxygen in air. Any way, the correct decomposition reaction; 2KClO3 (s) ----------> 2KCl (s) + 3O2 (g) For 3 moles of O2, we need 2 moles of KClO3 For 15 moles of O2, we need; 2 mol KClO3 x (15 mol O2 / 3 mol O2) = 10 mol KClO3

first you need to balance the reaction equation that is given; 2KClO3 -> 2K + 2ClO + 2O2 (decomposition reaction) thus, according to the balanced reaction equation, the mole ratio between KClO3 and O2 is 2:2 (or 1:1 if you simplify.) Thus, you are right - 15 mol of oxygen gas will be produced from 15 moles of KClO3. Hope this helps:-D

first you need to balance the reaction equation that is given; 2KClO3 -> 2K + 2ClO + 2O2 (decomposition reaction) thus, according to the balanced reaction equation, the mole ratio between KClO3 and O2 is 2:2 (or 1:1 if you simplify.) Thus, you are right - 15 mol of oxygen gas will be produced from 15 moles of KClO3. Hope this helps:-D

👍 60 | 👎 -5

Scarring is a major factor when it comes to removing a mole, most scarring occurs when the mole is cut from the skin. I didn't want to have my moles removed with a scalpel nor did I want any scarring, so I had to look around for another option. I found a product called Dermatend that uses only natural ingredients and in their case study there is a 98.6% chance of NO SCARRING. I ended up buying Dermatend because it also comes with a 100% guarantee and I can use it at home. I have removed 6 moles from my body so far and 1 of them was on my face, all the moles I have removed have left no scar. After they were gone I just applied a healing ointment I had around the house. I bought Dermatend from www.mole-wartremoval.com which is a web store by amazon.com, for me buying from such a large website made my purchasing easier.

my frnd got her removed, although it was not as huge as you describe, but she didn't had any scars? so not sure, but if it is not visible,let it be ther

If you have your own answer to the question how to write a decomposition reaction, then you can write your own version, using the form below for an extended answer.