ZuoTi.Pro
Question

Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2(g) = CO(g) + Br2(g) Kc is 0.190 at 73 °C. If you place 0.51The equilibrium constant for the dissociation of iodine molecules to iodine atoms 12(g) = 2 (g) is 3.76 x 10-3 at 1000 K. Sup

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

② Given data → Ke= 0.190, V IL COBra (2) - Colg) at Bra Initicel no. of mores 0.514 No. of moles at quilibrium (0.514-4) ActiAut equilibrium [cobr] = 0.514 - 0.232. [Corby = 0.202 male [co] = 0.232 mal/L & [Brg] = 0.232 mol/l & Given datar Ke= 3.7681442 = (0.330-2) X 18.5 X 0.00376 43° 0.0236 -0.07% 422 +0.072-0.0236 x = -0.07 10.07) - 4X4X (-010236) 284 = -0.07+ 0.0049 +0

0 0
Add a comment
Know the answer?
Add Answer to:
Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2(g) = CO(g) + Br2(g) Kc is 0.190 at 73 °C. If you plac...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Question 16 (Mandatory) (4.256 points) Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2(g) = CO(g)...

    Question 16 (Mandatory) (4.256 points) Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2(g) = CO(g) + Br2(g) Kc is 0.19 at 73 °C. If an initial concentration of 0.63 M COBr2 is allowed to equilibrate, what are the equilibrium concentrations of COBr2, CO, and Br2? Oa) (COBr2] = 0.30 M, [CO] = 0.33 M, (Bra] = 0.33 M Ob) (COBr2] = 0.63 M, [CO] = 0.35 M, (Br2] = 0.35 M Oc) [COBr2] = 0.11 M, [CO] = 0.26...

  • Carbonyl bromide can dissociate into carbon monoxide and bromine: COBr2(g) = (double arrow) CO(g) + Br2(g)...

    Carbonyl bromide can dissociate into carbon monoxide and bromine: COBr2(g) = (double arrow) CO(g) + Br2(g) At 73 °C, the equilibrium constant in terms of pressures, Kp, for this dissociation reaction is 5.40. (a) If 18.54 g of carbonyl bromide is placed in a 17.59-L vessel and heated to 73 °C, what is the partial pressure of carbon monoxide when equilibrium is attained? atm (b) What fraction of carbonyl bromide is dissociated at equilibrium?

  • carbonyl bromide, COBr2, decomposes to CO and Br2 with an Kc= .190 . A .015 mole...

    carbonyl bromide, COBr2, decomposes to CO and Br2 with an Kc= .190 . A .015 mole sample of carbonyl bromide is place in a 2.5 L flask. what will be the equilibrium concentrations of the reaction?

  • A more challenging blue-numbered questions answered in Appendix R 749 2 at *17. Carbonyl bromide decomposes...

    A more challenging blue-numbered questions answered in Appendix R 749 2 at *17. Carbonyl bromide decomposes to carbon monoxide and bromine. COBr2(g) 2 CO(g) + Br2(g) K is 0.190 at 73 °C. If you place 0.500 mol of COBro in a 2.00-L flask and heat it to 73 °C, what are the equilib- rium concentrations of COBr, CO, and Bry? What percentage of the original COBr, decomposed at this temperature? L i nkuee in water but its solubility in a...

  • Question 20 Carbonyl bromide decomposes to carbon monoxide and bromine according to the following reaction. COBr2(g)...

    Question 20 Carbonyl bromide decomposes to carbon monoxide and bromine according to the following reaction. COBr2(g) e2 CO(g) + Br2(g). A H = 30 kJ Which one of the changes below would cause the equilibrium to shift to the left? o'a. Decrease the container volume b. Increase the temperature C. Remove some Br2 d. Decrease the pressure e. Add some COBr2(g) Question 19 Find the pH of a 0.135 M aqueous solution of hypobromous acid (HOBr), for which Ka =...

  • Equal amounts of carbon monoxide and bromine react at 70° C to form carbonyl bromide. CO...

    Equal amounts of carbon monoxide and bromine react at 70° C to form carbonyl bromide. CO (g) + Br2 (g) <-->COBr2 (g) a) What is the equilibrium constant Kp at this temperature of the reaction when there is 47.2 volume-% of carbon monoxide in the equilibrium mixture and the total pressure in the equilibrium mixture is 1.0 MPa? Give the answer to four decimal places. The balance equation unit does not need to be written into the answer. (use partial...

  • Consider the equilibrium between COBr2, CO and Br2. COBr2(g) CO(g) + Br2(g) K = 0.254 at...

    Consider the equilibrium between COBr2, CO and Br2. COBr2(g) CO(g) + Br2(g) K = 0.254 at 350 K The reaction is allowed to reach equilibrium in a 6.40-L flask. At equilibrium, [COBr2] = 0.294 M, [CO] = 0.274 M and [Br2] = 0.274 M. (a) The equilibrium mixture is transferred to a 12.8-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a...

  • Consider the equilibrium between COBr2, CO and Br2. COBr2(g) -->CO(g) + Br2(g) K = 1.84 at...

    Consider the equilibrium between COBr2, CO and Br2. COBr2(g) -->CO(g) + Br2(g) K = 1.84 at 380 K The reaction is allowed to reach equilibrium in a 13.8-L flask. At equilibrium, [COBr2] = 3.02×10-2 M, [CO] = 0.236 M and [Br2] = 0.236 M. (a) The equilibrium mixture is transferred to a 6.90-L flask. In which direction will the reaction proceed to reach equilibrium? _________to the right? to the left? (b) Calculate the new equilibrium concentrations that result when the...

  • Consider the equilibrium between COBr2, CO and Br2 COBr2(g) at 382 K CO(g) + Brz(9) K=...

    Consider the equilibrium between COBr2, CO and Br2 COBr2(g) at 382 K CO(g) + Brz(9) K= 2.08 The reaction is allowed to reach equilibrium in a 13.8-L flask. At equilibrium, [COBr2] = 4.43x10-2 M, [CO] = 0.304 M and [Br2] = 0.304 M. (a) The equilibrium mixture is transferred to a 6.90-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 6.90-L...

  • 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 0.0458 mol of I2 in a 2.32−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

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT