What mass of potassium nitrate would you have in order to produce 1.00dm of oxygen at rtp?
Use PV = nRT; substitute rtp conditions and solve for n.
Then 2KNO3 ==> 2KNO2 + O2
You know mols O2 from above. Then
mols KNO3 = mols O2 from above x (2 mol KNO3/2 mols O2).
Finally, grams KNO3 = mols KNO3 x molar mass KNO3.
To determine the mass of potassium nitrate required to produce 1.00 dm³ of oxygen at room temperature and pressure (rtp), we need to consider the balanced equation for the decomposition of potassium nitrate:
2 KNO₃ → 2 KNO₂ + O₂
According to the equation, 2 moles of potassium nitrate produce 1 mole of oxygen gas. The molar volume of any gas at rtp is 22.4 dm³.
Step 1: Calculate the number of moles of oxygen gas required:
1.00 dm³ of oxygen gas is equivalent to 1.00/22.4 = 0.0446 moles of oxygen.
Step 2: Determine the number of moles of potassium nitrate needed:
Since the molar ratio between potassium nitrate and oxygen is 2:1, we need twice as many moles of potassium nitrate.
Therefore, the number of moles of potassium nitrate required is 2 * 0.0446 = 0.0892 moles.
Step 3: Calculate the molar mass of potassium nitrate:
The molar mass of potassium nitrate (KNO₃) can be calculated by adding the atomic masses of potassium (K), nitrogen (N), and oxygen (O):
K: 39.10 g/mol, N: 14.01 g/mol, O: 16.00 g/mol
Molar mass of KNO₃ = (39.10 + 14.01 + (3 * 16.00)) = 101.10 g/mol.
Step 4: Calculate the mass of potassium nitrate:
To find the mass of 0.0892 moles of potassium nitrate, multiply the number of moles by the molar mass:
Mass = 0.0892 moles * 101.10 g/mol = 9.02 grams (rounded to two decimal places).
Therefore, you would need approximately 9.02 grams of potassium nitrate to produce 1.00 dm³ of oxygen at rtp.
To determine the mass of potassium nitrate required to produce 1.00 dm³ of oxygen at RTP (room temperature and pressure), you need to follow these steps:
Step 1: Write the balanced chemical equation.
The formula for potassium nitrate is KNO₃. When it decomposes, it produces oxygen gas (O₂) and potassium nitrite (KNO₂).
2KNO₃(s) → 2KNO₂(s) + O₂(g)
Step 2: Find the molar ratio between potassium nitrate and oxygen.
From the balanced chemical equation, we can see that 2 moles of potassium nitrate are required to produce 1 mole of oxygen.
Step 3: Determine the molar volume of a gas at RTP.
At RTP (room temperature and pressure), 1 mole of any ideal gas occupies 22.4 dm³.
Step 4: Calculate the number of moles of oxygen.
Since we want to produce 1.00 dm³ of oxygen, we know that this corresponds to 1 mole because the molar volume of a gas at RTP is 22.4 dm³.
Step 5: Use the molar ratio to find the number of moles of potassium nitrate.
Since we know that 2 moles of potassium nitrate produce 1 mole of oxygen, the number of moles of potassium nitrate required can be found by multiplying the number of moles of oxygen by the ratio.
Step 6: Calculate the molar mass of potassium nitrate.
The molar mass of KNO₃ is the sum of the atomic masses of the constituent elements: potassium (K), nitrogen (N), and oxygen (O). Look up the atomic masses and calculate the sum.
Step 7: Calculate the mass of potassium nitrate.
To calculate the mass of potassium nitrate needed, multiply the number of moles of potassium nitrate by the molar mass of KNO₃.
Following these steps, you can determine the mass of potassium nitrate required to produce 1.00 dm³ of oxygen at RTP.