potassium chlorate can be thermally decomposed to oxygen and potassium chloride. calculate the mass of potassium chlorate that must be decomposed by heat to produce 10.0L of oxygen gas at 150 degrees celsius and 150 kPa pressure
2KClO3 ==> 2KCl + 3O2
You need how many mols O2? That's
n = PV/RT. Substitute and solve for n = mols O2.
Using the coefficients in the balanced equation, convert mols O2 needed to mols KClO3.
Convert mols KClO3 to g KClO3 needed. That's grams = mols x molar mass = ?
To calculate the mass of potassium chlorate required to produce 10.0L of oxygen gas at 150 degrees Celsius and 150 kPa pressure, we need to use the ideal gas law equation and the balanced chemical equation for the decomposition of potassium chlorate.
The balanced chemical equation for the thermal decomposition of potassium chlorate (KClO3) is:
2 KClO3(s) → 2 KCl(s) + 3 O2(g)
Step 1: Calculate the moles of oxygen gas:
Since we have the volume (10.0L), temperature (150 degrees Celsius which needs to be converted to Kelvin), and pressure (150 kPa), we can use the ideal gas law equation: PV = nRT.
Convert the temperature to Kelvin: 150 degrees Celsius + 273.15 = 423.15 K.
R is the ideal gas constant which is 0.0821 L·atm/(mol·K).
Now, plug the values into the equation:
PV = nRT
n = (PV) / (RT)
n = (150 kPa * 10.0L) / (0.0821 L·atm/(mol·K) * 423.15 K)
Step 2: Determine the stoichiometry between oxygen gas and potassium chlorate:
From the balanced equation, we know that 2 moles of KClO3 produce 3 moles of O2, so we need to find the moles of O2 and multiply it by the ratio of potassium chlorate to oxygen gas.
Step 3: Calculate the mass of potassium chlorate:
To calculate the mass of potassium chlorate, multiply the moles of O2 by the molar mass of KClO3.
Molar mass of KClO3:
K = 39.10 g/mol
Cl = 35.45 g/mol
O = 16.00 g/mol
Molar mass of KClO3 = 39.10 g/mol + 35.45 g/mol + (3 * 16.00 g/mol)
Finally, multiply the moles of O2 by the molar mass of KClO3 to determine the mass of potassium chlorate.
It's important to remember that this calculation assumes ideal conditions and a complete reaction, so actual experimental conditions may lead to slightly different results.