100% satisfaction guarantee Immediately available after payment Both online and in PDF No strings attached
logo-home
Previously searched by you
Previously searched by you
logo
Summary AQA A-Level Chemistry 1.10 Equilibrium Constant Kp £2.99   Add to cart
Quickly navigate to
Preview
  2.  
  3. AQA
  4.  
  5. Chemistry
  6.  
  7. 3.1.10 Kp

Summary

Summary AQA A-Level Chemistry 1.10 Equilibrium Constant Kp
 15 views  0 purchase
  • Institution
  • AQA

These are detailed Revision Notes for Topic 1.10 of AQA A-Level Chemistry (Kp). They were written by me using a combination of the textbook and class notes. I will also be uploading the other topics and creating bundles. Topics Included: - Equilibrium constant Kp for homogenous systems

Preview 1 out of 1  pages

Document information

  • No
  • Chapter 19
  • May 8, 2022
  • 1
  • 2021/2022
  • Summary

Subjects

Connected book

book image

Book Title:

Author(s):

  • Edition:
  • ISBN:
  • Edition:

More summaries for

All for this textbook (24)

Written for

All documents for this subject (1)

Seller

avatar-seller
emilysarahjudge

Reviews received

Content preview

Equilibrium Constant, Kp
19.1 Equilibrium Constant Kp for Homogeneous Systems:
19.1 Equilibrium constant
- Many reversible reactions take place in the gas phase.
- Gaseous equilibria also obey the equilibrium law, but it is usual to express their Kp for homogeneous
concentrations in a different way using the idea of partial pressure. systems
!"#$% "' ()% *
- The mole fraction of gas A = +"+)# !"#$% "' ()%
- The partial pressure of a gas in a mixture is found by multiplying the mole fraction of that gas by the
total pressure.
- Partial pressure of gas A = mole fraction of A x total pressure
- It is worked out the same way as Kc but using the partial pressures rather than concentrations.
e.g., 1.00 moles of PCl5 vapour are heated to 500K in a sealed vessel. The equilibrium
mixture, at a pressure of 625kPa, contains 0.600 moles of chlorine. Calculate Kp

PCl5 ⇌ PCl3 + Cl2
Initial mol 1.00 0.00 0.00
Change mol -0.600 +0.600 +0.600
Equilibrium mol 0.400 0.600 0.600
Mol fraction 0.25 0.375 0.375
Partial pressure 156.25 234.375 234.375

(𝑃𝐶𝑙- )(𝐶𝑙. ) 234.375 × 234.375
𝐾, = =
(𝑃𝐶𝑙/ ) 156.25
Kc = 352 kPa

- It is affected by Le Chatelier’s principle in the same way as Kc. Increasing the temperature of an
exothermic reaction pushes the equilibrium to the left and decreases Kp

The benefits of buying summaries with Stuvia:

Guaranteed quality through customer reviews

Guaranteed quality through customer reviews

Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.

Quick and easy check-out

Quick and easy check-out

You can quickly pay through credit card for the summaries. There is no membership needed.

Focus on what matters

Focus on what matters

Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!

Frequently asked questions

What do I get when I buy this document?

You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.

Satisfaction guarantee: how does it work?

Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.

Who am I buying these notes from?

Stuvia is a marketplace, so you are not buying this document from us, but from seller emilysarahjudge. Stuvia facilitates payment to the seller.

Will I be stuck with a subscription?

No, you only buy these notes for £2.99. You're not tied to anything after your purchase.

Can Stuvia be trusted?

4.6 stars on Google & Trustpilot (+1000 reviews)

64438 documents were sold in the last 30 days

Founded in 2010, the go-to place to buy revision notes and other study material for 14 years now

Start selling
£2.99
  • (0)
  Add to cart