Question

2 of 2 exercise Iodine and bromine react to give iodine monobromide IBr. I2(g) + Br2(g)...

2 of 2 exercise

Iodine and bromine react to give iodine monobromide IBr.

I2(g) + Br2(g) ----- 2IBr(g)

What is the equilibrium composition of a mixture at 132°C that initially contained 2.30*10^-3 mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant Kc for this reaction at 132°C is 82.3

[I2] = M

[Br2] = M

[IBr] = M

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Iodine and bromine react to give iodine monobromide, IBr. I2(g) + Br2(g) 2 IBr(g) What is...
Iodine and bromine react to give iodine monobromide, IBr. I2(g) + Br2(g) 2 IBr(g) What is the equilibrium composition of a mixture at 154°C that initially contained 1.10×10-3 mol each of iodine and bromine in a 5.0 L vessel? The equilibrium constant Kc for this reaction at 154°C is 130. please show steps
Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc =...
Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 102 This reaction mixture contains initially 0.41 M I2 and 0.27 M Br2. Calculate the equilibrium concentration of I2, Br2, and IBr?
At 25.0°C, the equilibrium constant Kc for Br2(g) + I2 <=> 2IBr(g) is 282. If the...
At 25.0°C, the equilibrium constant Kc for Br2(g) + I2 <=> 2IBr(g) is 282. If the initial concentration of bromine is 0.0100M, of Iodine is 0.0100M and of iodine monobromide is 0.200M, what is the equilibrium concentration of IBr?
Constants | Periodic Table For the reaction I2(g)+Br2(g)←−→2IBr(g), Kc=280 at 150 ∘C. Suppose that 0.500 mol...
Constants | Periodic Table For the reaction I2(g)+Br2(g)←−→2IBr(g), Kc=280 at 150 ∘C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150 ∘C. Part A Part complete What is the equilibrium concentration of IBr? 0.223   M   SubmitPrevious Answers Correct Part B What is the equilibrium concentration of I2? nothing   M   SubmitPrevious AnswersRequest Answer Incorrect; Try Again Part C What is the equilibrium concentration of Br2? nothing   M  
For the equilibrium 2IBr(g)?I2(g)+Br2(g) Kp=8.5×10?3 at 150 ?C. If 2.3×10?2 atm of IBr is placed in...
For the equilibrium 2IBr(g)?I2(g)+Br2(g) Kp=8.5×10?3 at 150 ?C. If 2.3×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached?
For the equilibrium 2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 at 150 ∘C. Part A If 2.1×10−2 atm of IBr is...
For the equilibrium 2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 at 150 ∘C. Part A If 2.1×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? Express your answer to two significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B If 2.1×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? Express your answer to two significant figures and include...
2IBr <-- --> I2 + Br2. (The arrows are overlapping each other not sure how to...
2IBr <-- --> I2 + Br2. (The arrows are overlapping each other not sure how to do that) the equilibrium constant Kc at 100 degrees C is 0.026. If 2.40 x 10^-2 mol IBr is placed in a .800-L vessels at 100 degrees C, what is the molarities at equilibrium in the vapor? A) IBr____M. B) I2____M. C) Br2____M.
The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000...
The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 × 10−5. Suppose you start with 0.0454 mol of I2 in a 2.28−L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2? M What is the equilibrium concentration of I? M
The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000...
The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 × 10−5. Suppose you start with 0.0454 mol of I2 in a 2.35−L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2? M What is the equilibrium concentration of I? M
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT