Answer:
0.16 L
Explanation:
Step 1: Write the balanced equation
C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g)
Step 2: Calculate the moles of CO₂ produced from 0.012 moles of O₂
The molar ratio of O₂ to CO₂ is 5:3. The moles of CO₂ produced are 3/5 × 0.012 mol = 0.0072 mol.
Step 3: Calculate the volume occupied by 0.0072 moles of CO₂ at standard temperature and pressure
At STP, 1 mole of CO₂ occupies 22.4 L.
0.0072 mol × 22.4 L/1 mol = 0.16 L
HOPE THAT HELP YOU mark me brinilylist
Answer:
sorry but we can't answer without the pic
Explanation:
there is not context random people cant solve this because there is no way to know what the chart means and also don't fake 40 points. I'm sorry but if you can add context I might be able to help :/
Answer:
4204 K
Explanation:
Step 1: Data
<em>Given data</em>
- Density of uranium hexafluoride (ρ): 0.5820 g/L
- Pressure of uranium hexafluoride (P): 0.5073 atm
<em>Required data</em>
- Universal gas constant (R): 0.08206 atm.L/mol.K
- Molar mass of uranium hexafluoride (M): 352.02 g/mol
Step 2: Calculate the temperature of the gas
We will use the following expression derived from the ideal gas equation.
P × M = ρ × R × T
T = P × M/ρ × R
T = 0.5073 atm × (352.02 g/mol)/(0.5820 g/L) × (0.08206 atm.L/mol.K)
T = 4204 K
