The equilibrium constant for the following reaction is 79.8 at a certain temperature. 4 A(g) + B2(g) 3 C(g) 0.100 mol of A and 0.150 mol of B are present at equilibrium in a 4.00-L flask. What is the molar concentration of C in the flask at equilibrium?
Added by Jonathan M.
Step 1
The reaction is: \[ 4 A(g) + B_2(g) \rightleftharpoons 3 C(g) \] The equilibrium constant expression is given by: \[ K_c = \frac{[C]^3}{[A]^4[B_2]} \] Show more…
Show all steps
Your feedback will help us improve your experience
Adi S 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
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g) ↽−−⇀ 4C(g) 𝐾c = 1.53 × 1031 If, at this temperature, 1.60 mol of A and 3.60 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A]= ___ M [B]= ___ M [C]= ___ M
Adi S.
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3 A(g) + 2 B(g) ⇌ 4 C(g) Kc = 2.13 × 10^31 If, at this temperature, 1.00 mol of A and 3.80 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = 0.33 M [B] = 3.13 M [C] = 1.33 M
Dj T.
Brooke 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