Answered

At Westonci.ca, we provide clear, reliable answers to all your questions. Join our vibrant community and get the solutions you need. Discover detailed solutions to your questions from a wide network of experts on our comprehensive Q&A platform. Experience the convenience of finding accurate answers to your questions from knowledgeable experts on our platform.

Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 5.0L flask with 4.5 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.1 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

Sagot :

Answer:

Kp = 7.4727

Explanation:

Let's write the balanced equilibrium reaction:

2NH₃ <-------> N₂ + 3H₂     Kp = ??

Now, if we want to calculate the Kp, we need to write an ICE chart with this reaction, which is the following:

         2NH₃ <-------> N₂ + 3H₂  

I.         4,5                 0        0

C.       -2x                +x     +3x

E.        4,5-2x            x       3x

According to this chart, the Kp expression should be:

Kp = (PH₂)³ * (PN₂) / (PNH₃)²   (1)

The value of x, we already know it because the problem states that the amount of nitrogen gas is 1.1 atm, so replacing this value into (1) we have:

Kp = (3*1.1)³ * (1.1) / (4.5 - (2 * 1.1))²

Kp = 39.5307 / 5.29

Kp = 7.4727

Hope this helps

Thank you for trusting us with your questions. We're here to help you find accurate answers quickly and efficiently. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Stay curious and keep coming back to Westonci.ca for answers to all your burning questions.