Question

1. A mixture of 3.00 mol of Cl2 and 3.00 mol of H20 are enclosed in a 5.00-L flask at equilibrium, 3.00% of the C12 has been
0 0
Add a comment Improve this question Transcribed image text
Answer #1

we lume place s le 3 Velum e 0- 6-44 hars been Censu med o Foo now the balanadreaction ne have atequn 0,6-o.ors o.61. о. о13Ku 2.9S 2. 子

Add a comment
Know the answer?
Add Answer to:
1. A mixture of 3.00 mol of Cl2 and 3.00 mol of H20 are enclosed in...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • A mixture of 3.00 mol of Cl2 and 3.00 mol of CO is enclosed in a 5.00-L flask at 600.°C. At equil...

    A mixture of 3.00 mol of Cl2 and 3.00 mol of CO is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2(g) = COCl2(g) Calculate Kc for the reaction at 600.°C. Calculate deltaG for the reaction at this temperature. = kJ/mol CO(g)= deltaH= -110.5 (kJ/mol) deltaG= -137.2 (kj/mol) S= 197.7 (j/molK) Cl2(g)= S= 223.1 J/molK COCl2(g)= deltaH= -218.8(kJ/mol) deltaG= -204.6 (kj/mol) S= 197.7 J/molK

  • I don't get how to do 5 or or co2, 0.750 mol of H20, and 1.00...

    I don't get how to do 5 or or co2, 0.750 mol of H20, and 1.00 mol of CO to a 5.00 L reactor at 990 CO2 (g) + H2 (g) H2O (g) + CO (g) 5. At 35°C, the equilibrium constant (Kc) for the reaction below is 1.6x 10. An equilibrium mixture was found to have the following concentrations of Cl2 and NOCI: [Cl2] = 1.2 x 10-2 M; [NOCl] = 2.8 × 10-1 M. Calculate the concentration of...

  • A mixture of 0.008603 mol of Cl2, 0.05744 mol of H2O, 0.05353 mol of HCl, and...

    A mixture of 0.008603 mol of Cl2, 0.05744 mol of H2O, 0.05353 mol of HCl, and 0.06453 mol of O2 is placed in a 1.0-L steel pressure vessel at 1529 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.006795 mol of Cl2 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. Peq(Cl2) =  . Peq(H2O) =  . Peq(HCl) =  . Peq(O2) =  . (b) Calculate...

  • A mixture of 0.1468 mol of Cl2, 0.04712 mol of H2O, 0.02609 mol of HCl, and...

    A mixture of 0.1468 mol of Cl2, 0.04712 mol of H2O, 0.02609 mol of HCl, and 0.1672 mol of O2 is placed in a 1.0-L steel pressure vessel at 579 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.006984 mol of HCl is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. Peq(Cl2) = ? Peq(H2O) = ? Peq(HCl) = ? Peq(O2)...

  • A mixture of 0.482 M H20, 0.419 M Cl20, and 0.748 M HCIO are enclosed in...

    A mixture of 0.482 M H20, 0.419 M Cl20, and 0.748 M HCIO are enclosed in a vessel at 25 °C. (Reaction) H2O(g) + C12O (g) <------> 2HOCI(g) Kc = 0.090 at 25 °C Calculate the equilibrium concentrations of each gas at 25 °C [H2O] = M [Cl2O] = M [HOCL]= M

  • 5-7 (ACS-style) A mixture of 2.0 mol of CO (g) and 2.0 mol of H20 (g) was allowed to come to equilibrium in a 10.0-L fl...

    5-7 (ACS-style) A mixture of 2.0 mol of CO (g) and 2.0 mol of H20 (g) was allowed to come to equilibrium in a 10.0-L flask at a high temperature. If Kc = 4.0, what is the molar concentration of H2 (g) in the equilibrium mixture? The equation for the reaction is: CO(g) + H20 (g) 5 CO2(g) + H2 (g) A) 0.67 M B) 0.40 M C) 0.20 M D) 0.13 M

  • I NEED A COMPLETE AND CLEAR SOLUTION PLEASE! thanks A mixture of 0.10 mol of NO,...

    I NEED A COMPLETE AND CLEAR SOLUTION PLEASE! thanks A mixture of 0.10 mol of NO, 0.050 mol of H2 and 0.10 mol of H2O is placed in a 1.0-L flask and allowed to reach equilibrium as shown below: 2 NO (g) +2 H(g)N2 (g) + 2 H2O (g) At equilibrium [NO] = 0.062 M. Calculate the equilibrium constants Kc and Kp for this reaction.

  • Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K...

    Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K The reaction is allowed to reach equilibrium in a 15.2-L flask. At equilibrium, [PCIs]-9.75x102 M, [PCl,]-o.156 M and [C12] = 0.156 M. (a) The equilibrium mixture is transferred to a 7.60-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 7.60-L flask. [PCI5] [C12] =

  • A mixture of 0.5540 M CO and 0.3180 M Cl2 is enclosed in a vessel and...

    A mixture of 0.5540 M CO and 0.3180 M Cl2 is enclosed in a vessel and heated to 1000 K. cog) +Cl2(g) 근 COC12(g) Kc =255.0 at 1000 K Calculate the equilibrium concentration of each gas at 1000 K. Number Number Number

  • A mixture of 0.1148 mol of O2, 0.03185 mol of NOCI, 0.1467 mol of NO2, and...

    A mixture of 0.1148 mol of O2, 0.03185 mol of NOCI, 0.1467 mol of NO2, and 0.2587 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 436 K. The following equilibrium is established: 102(9) + 2 NOCI(9) = 2 NO2(g) + 1 C12(9) At equilibrium 0.008912 mol of NOCI is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of O2, NOCI, NO, and Cl2. Peq(O2) = x . Pea(NOCI) = Peg(NO2) = x ....

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