CALCULATE THE NUMBERS OF MOLES OF POTASSIUM CHLORATE THAT MUST DECOMPOSE TO PRODUCE POTASSIUM CHLORIDE AND 1.80 MOLES OF GLYCOGEN GAS
Here is a link for solving stoichiometry problems; HOWEVER, I don't know how in the world you intend to get glycogen out of KClO3. There must be more to the problem than what you've posted.
http://www.jiskha.com/science/chemistry/stoichiometry.html
stoichiometrt
To calculate the number of moles of potassium chlorate required to produce potassium chloride and 1.80 moles of glycol gas, we first need to write the balanced chemical equation for the decomposition of potassium chlorate.
The balanced chemical equation for the decomposition of potassium chlorate is:
2KClO3 -> 2KCl + 3O2
From the balanced equation, we can see that 2 moles of potassium chlorate decompose to give 2 moles of potassium chloride and 3 moles of oxygen gas.
We are given that 1.80 moles of glycol gas is produced during the decomposition. Since there is no direct relationship between glycol gas and potassium chlorate in the balanced equation, we can ignore it for the purpose of calculating the moles of potassium chlorate.
Therefore, we can conclude that for every 2 moles of potassium chlorate, we obtain 2 moles of potassium chloride.
Hence, to calculate the number of moles of potassium chlorate required, we can use the following formula:
moles of potassium chlorate = (1.80 moles of glycol gas) x (2 moles of potassium chlorate/2 moles of potassium chloride)
Simplifying the equation, we find:
moles of potassium chlorate = 1.80 moles of glycol gas
Therefore, the number of moles of potassium chlorate required to produce potassium chloride and 1.80 moles of glycol gas is also 1.80 moles.
To calculate the number of moles of potassium chlorate (KClO3) needed to produce potassium chloride (KCl) and 1.80 moles of glycol gas (presumably carbon monoxide, CO), you would need to use the balanced chemical equation for the decomposition of potassium chlorate.
The balanced chemical equation for the decomposition of potassium chlorate is:
2KClO3(s) ⟶ 2KCl(s) + 3O2(g)
From the balanced equation, we can see that 2 moles of KClO3 produce 2 moles of KCl. However, we are given the number of moles of CO, which is not directly related to KClO3.
To understand how many moles of KClO3 are required, we need to determine the stoichiometry between KClO3 and CO. Unfortunately, the information provided does not include this stoichiometric relationship. Therefore, we cannot directly calculate the number of moles of KClO3 needed.
If you have the stoichiometric coefficients of the reaction between KClO3 and CO, please provide them. Without the exact stoichiometry, it is not possible to calculate the moles of KClO3 necessary to produce the given quantity of CO.