calculate the mass of potassium chlorate required to produce 35 g of potassium chloride on complete decomposition
Answers
Answer: 57.55 g
Explanation
1. Write the balanced equation
2. Calculate the atomic mass
3. From the equation we can find that to produce 149 g of KCL we need 245 g of .
Hence, 149 g of is produced by g of .
1 g of is produced by g of .
35 g of is produced by g of .
Answer:
Step-by-step explanation:
Assuming complete thermal decomposition of KClO3 i.e. potassium chlorate the following reaction takes place…
2KClO3 → 2KCl + 3O2
Hence it's clearly visible that the molar ration between KClO3 and O2 is 2:3. Intuitively speaking u need 2 mol of compound to react with 3 mol of O2.
Now the molar volume at STP for an ideal gas is 22.4 dm3/mol (assuming O behaves ideally we shall take this number). Intuitively speaking one mol of ideal gas occupies 22.4 dm3 volume. Hence if u have 6.72 dm3 of ideal gas u have 0.3 mol of that gas (6.72/22.4).
Since we have the molar ratio as 2:3 and we have no of moles of O2 as 0.3, the no of moles of KClO3 can be calculated and it turns out to be 0.2 mol.
Mass = No. Of moles * Molar mass ofor substance
Molar mass of KClO3 is roughly 122.5 g/mol.
Hence the mass required will be = 0.2 mol *122.5 g/mol
And u get the mass as 24.5 g
Hope this works…