Question

for the reaction, Br2(g) ⇌ 2Br(g) the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C....

for the reaction,

Br2(g) ⇌ 2Br(g)

the equilibrium constant, Kc is 1.10 × 10−3 at 1280°C. Determine the initial and equilibrium concentrations of Br if the initial and equilibrium concentrations of Br2 are 5.70 ×10−3 M and 5.30 × 10−3M, respectively.


Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The equilibrium constant Kc for the reaction below is 0.00173 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00173 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0393 M and [Br] = 0.0940 M, calculate the concentrations of these species at equilibrium. [Br2] = M [Br] = M
The equilibrium constant Kc for the reaction below is 0.00431 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00431 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0668 M and [Br] = 0.0466 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant Kc for the reaction below is 0.00622 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00622 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0672 M and [Br] = 0.0563 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant Kc for the reaction below is 0.00440 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00440 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0131 M and [Br] = 0.0854 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant Kc for the reaction below is 0.00967 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00967 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0427 M and [Br] = 0.0554 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant Kc for the reaction below is 0.00399 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00399 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0395 M and [Br] = 0.0655 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730°...
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730° C. Starting with 4.20 moles of HBr in a 17.8−L reaction vessel, calculate the concentrations of H2,Br2, and HBr at equilibrium. 17. The equilibrium constant Kc for the reaction below is 0.00771 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0433 M and [Br] = 0.0462 M, calculate the concentrations of these species at equilibrium. For the reaction...
Be sure to answer all parts. The equilibrium constant Kc for the reaction below is 0.00599...
Be sure to answer all parts. The equilibrium constant Kc for the reaction below is 0.00599 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0344 M and [Br] = 0.0508 M, calculate the concentrations of these species at equilibrium. [Br2] = M [Br] = M
Be sure to answer all parts. The equilibrium constant Kc for the reaction below is 0.00180...
Be sure to answer all parts. The equilibrium constant Kc for the reaction below is 0.00180 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0736 M and [Br] = 0.0751 M, calculate the concentrations of these species at equilibrium. [Br2] = ___M [Br] =____ M
If you take the following chemical equation: Br2(g)   --->   2Br(g) The Kc is 8.08 x 10...
If you take the following chemical equation: Br2(g)   --->   2Br(g) The Kc is 8.08 x 10 -4 for the temperature of 1756K. If the initial concentration of Br2(g) was 3.2M, what are the equilibrium concentrations? If after you get to equilibrium you add an extra 1.3M of Br2, what is the Q value and what would be the new equilibrium concentrations?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT