The reaction 2NO (g) + Br2 (g) ⇌ 2NOBr (g) has KP = 109 at 25°C. Ifthe equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.
Added by Michael D.
Step 1
Step 1: Write down the equilibrium constant expression for the reaction: \[ K_p = \frac{(P_{NOBr})^2}{(P_{NO})(P_{Br_2})} \] Show more…
Show all steps
Your feedback will help us improve your experience
Syon Schlecht and 80 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
onsider the reaction: 2NO(g)+Br2(g)⇌2BrNO(g)K=32.9 at 315 K In a reaction mixture at equilibrium, the partial pressure of NO is 119 mbar and that of Br2 is 129 mbar . Part A What is the partial pressure of BrNO in the equilibrium mixture?
Ronald P.
Consider the equilibrium: N2(g) + O2(g) + Br2(g) ⇌ 2NOBr(g) Calculate the equilibrium constant Kp for this reaction, given the following information (at 301 K): 2NO(g) + Br2(g) ⇌ 2NOBr(g) Kc = 2.2 2NO(g) ⇌ N2(g) + O2(g) Kc = 2.2 × 10^30
Adi S.
Br2(g) + 3F2(g) ⇌ 2BrF3(g) Kp = 5.4 x 10^8 Assume 0.37 atm Br2 and 0.42 atm F2 are placed in a container. They react according to the equation above. What is the pressure of F2 at equilibrium?
Alkendra S.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD