2 KClO3 -> KCL + 3O2
Molar weight of O2 = 32 grams/mole (so close it doesn't matter)
30 grams/32grams/mole = 0.9375 moles
Molar weight of KCL = 39+35.5 = 74.5 grams/mole (Want more accuracy? Do it yourself?)
now if we have 3 moles of O2 then we have 2 moles of KCl.
If we have one mole of O2 then we have 2/3 moles of KCL
What ever moles we have of O2 we must multiply it by 2/3 to get the moles of KCl
So we have 0.9375moles of O2 x 2/3 = 0.625 moles of KCl
So 0.625 moles of KCl x 74.5 grams/mole KCl = 46.5625 grams KCl
The equation that describes this process is as follows: 2KClO3 ---> 2KCl + 3O2 For every 2 moles of reactants consumed 3 moles of oxygen gas are produced. 3 mol O2 / 2 mol KClO3 = x mol O2 / 12.3 mol KClO3 x = 12.3 mol x 3 mol / 2 mol = 18.45 mol Therefore, 18.5 mol (3 significant figures) of oxygen are produced by the decomposition of 12.3 mol of potassium chlorate
2 grams of Oxygen can be obtained from 5 grams of KClO3 (only if the "CL" means "Cl", which is Chlorine! Remember that only the first letter of the atomic symbol is capitalized.)
Oh, dude, chemistry time! So, when 25 grams of potassium chlorate decompose, you get 74.55% potassium chloride and 25.45% oxygen. So, if you do the math, you'd get around 18.64 grams of potassium chloride. But hey, who's counting, right?
Alls you do to find a molar mass is add up all of the atomic masses. Potassium=39.09 Chlorine= 35.453 Oxygen(3)=15.999. So KClO3 would equal 271.65g to a mol? Then I think to find the number of atoms of each you would take the atomic mass * avacodo's number so it would be for example chlorine. 1gCl(35.453/1)(6.022*10^23/1) However I might be wrong on that part.
To calculate the mass of potassium chlorate containing 40.0g of oxygen, first determine the molar mass of oxygen (16g/mol). Then, use the molecular formula of potassium chlorate (KClO3) to find the oxygen's molar ratio in KClO3 (1:3). Finally, calculate the mass of KClO3 using the molar mass and the molar ratio to find that approximately 186 grams of potassium chlorate contain 40.0g of oxygen.
The equation that describes this process is as follows: 2KClO3 ---> 2KCl + 3O2 For every 2 moles of reactants consumed 3 moles of oxygen gas are produced. 3 mol O2 / 2 mol KClO3 = x mol O2 / 12.3 mol KClO3 x = 12.3 mol x 3 mol / 2 mol = 18.45 mol Therefore, 18.5 mol (3 significant figures) of oxygen are produced by the decomposition of 12.3 mol of potassium chlorate
2 grams of Oxygen can be obtained from 5 grams of KClO3 (only if the "CL" means "Cl", which is Chlorine! Remember that only the first letter of the atomic symbol is capitalized.)
Oh, dude, chemistry time! So, when 25 grams of potassium chlorate decompose, you get 74.55% potassium chloride and 25.45% oxygen. So, if you do the math, you'd get around 18.64 grams of potassium chloride. But hey, who's counting, right?
Alls you do to find a molar mass is add up all of the atomic masses. Potassium=39.09 Chlorine= 35.453 Oxygen(3)=15.999. So KClO3 would equal 271.65g to a mol? Then I think to find the number of atoms of each you would take the atomic mass * avacodo's number so it would be for example chlorine. 1gCl(35.453/1)(6.022*10^23/1) However I might be wrong on that part.
To calculate the mass of potassium chlorate containing 40.0g of oxygen, first determine the molar mass of oxygen (16g/mol). Then, use the molecular formula of potassium chlorate (KClO3) to find the oxygen's molar ratio in KClO3 (1:3). Finally, calculate the mass of KClO3 using the molar mass and the molar ratio to find that approximately 186 grams of potassium chlorate contain 40.0g of oxygen.
The molar mass of potassium chlorate (KClO3) is 122.55 g/mol. This means that 122.55 grams of potassium chlorate yield 3 moles of oxygen gas. To calculate the amount of potassium chlorate that decomposes to yield 30 grams of oxygen, you can set up a simple ratio using the molar masses.
This question seems to be about the reactant side of a chemical equation. To calculate the mass of oxygen produced, you need to know the stoichiometry of the reaction. Without that information, it is not possible to determine why 160 grams of oxygen would be produced.
The decomposition of potassium chlorate produces oxygen gas and potassium chloride. The molar ratio of oxygen to potassium chlorate is 3:2. Therefore, to find the grams of oxygen produced, you would calculate (6.02g * 3 mol O2/2 mol KClO3) * molar mass of O2.
When the amount of oxygen is limited, carbon and oxygen react to form carbon monoxide. How many grams of CO can be formed from 35 grams of oxygen?
To find the mass of water decomposed, we first need to calculate the total mass of the products formed, which is 4g (hydrogen gas) + 32g (oxygen gas) = 36g. The original mass of water decomposed is equal to the total mass of products formed, so 36g of water is decomposed.
To determine the amount of gas needed to react with 348.5 grams of oxygen, you need to know the balanced chemical equation of the reaction. Then, use the stoichiometry of the reaction to calculate the amount of gas required based on the molar ratio between the gas and oxygen in the reaction.
To calculate the number of grams of oxygen needed to react with 6.78 grams of ammonia, we first write out the balanced chemical equation for the reaction between ammonia (NH3) and oxygen (O2) to form nitrogen monoxide (NO) and water (H2O). Then we use the stoichiometry of the equation to find the molar ratio between ammonia and oxygen. Finally, we convert the mass of ammonia to moles and then use the molar ratio to find the mass of oxygen needed.