Top topic this week
Back to FAQs
Related FAQs
Frequently Asked Question
Questions asked by users might not always be phrased in the clearest way.
When heated PCl5, phosphorus pentachloride, forms PCl3 and Cl2 as follows:pcl5(g) pcl3(g) + Cl2(g)When 1.00 mol PCl5 in a 1.00-l container is allowed to come to equilibrium at 180 °c, the mixture is found to contain 0.135 mol. PCl3. What would be the molar composition of the mixture?the freezing point of PCl5 is 160.5 °c. What will be the partial pressures
Accepted Answer
Here's the breakdown:
1. Equilibrium Calculation:
- Initial: 1.00 mol PCl5, 0 mol PCl3, 0 mol Cl2
- Change: -0.135 mol PCl5, +0.135 mol PCl3, +0.135 mol Cl2 (based on the stoichiometry of the reaction)
- Equilibrium: 0.865 mol PCl5, 0.135 mol PCl3, 0.135 mol Cl2
2. Partial Pressures:
- Assuming ideal gas behavior, we can use the ideal gas law (PV = nRT) to find the partial pressures.
- Since the volume is 1.00 L and the temperature is constant, the partial pressure of each component is directly proportional to its molar amount.
- Partial Pressure of PCl5: (0.865 mol / 1.00 L)
R
(180 + 273.15 K) = ... (calculate the value)
- Partial Pressure of PCl3: (0.135 mol / 1.00 L)
R
(180 + 273.15 K) = ... (calculate the value)
- Partial Pressure of Cl2: (0.135 mol / 1.00 L)
R
(180 + 273.15 K) = ... (calculate the value)
3. Freezing Point:
- The freezing point of PCl5 (160.5 °C) is not directly relevant to the equilibrium calculation or the partial pressures at 180 °C. It's useful if you were investigating phase transitions or solid-state properties.
Articles you might like