Asked by Anonymous
The two common chlorides of Phosphorus, PCl3 and PCl5, both important in the production of other phosphorous compounds, coexist in equilibrium as shown in the balanced chemical reaction below:
PCl3 (g) + Cl2 (g) <-----> PCl5 (g)
At 250 C, an equilibrium mixture in a 2.50 L flask contains 0.305 g PCl5, 0.440 g PCl3, and 4.24 g Cl2.
A. Show the equilibrium Constant formula.
B. What is the value of Kc for this reaction? Hint: Use molarity in the Kc calculations.
My answers:
A.
Kc = [PCl5]/([Cl2][PCl3])
B.
1.826
PCl3 (g) + Cl2 (g) <-----> PCl5 (g)
At 250 C, an equilibrium mixture in a 2.50 L flask contains 0.305 g PCl5, 0.440 g PCl3, and 4.24 g Cl2.
A. Show the equilibrium Constant formula.
B. What is the value of Kc for this reaction? Hint: Use molarity in the Kc calculations.
My answers:
A.
Kc = [PCl5]/([Cl2][PCl3])
B.
1.826
Answers
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.