ZuoTi.Pro
Question

The equilibrium constant, Kc, for the following reaction is 5.89×10-4 at 635 K. NH4I(s)<-->NH3(g) + HI(g)...

The equilibrium constant, Kc, for the following reaction is 5.89×10-4 at 635 K.

NH4I(s)<-->NH3(g) + HI(g)


Calculate Kc at this temperature for the following reaction:

NH3(g) + HI(g) <-->NH4I(s)

Kc=?

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

Homework Answers

Answer #1

The given reaction is:

NH4I(s) <-> NH3(g) + HI(g)

Kc = [NH3][HI]

= 5.89*10^-4

The required reaction is:

NH3(g) + HI(g) <-> NH4I(s)

Use:

Kc’ = 1/([NH3][HI])

= 1/ Kc

= 1/(5.89*10^-4)

= 1.70*10^3

Answer: 1.70*10^3

0 0
Add a comment
Know the answer?
Add Answer to:
The equilibrium constant, Kc, for the following reaction is 5.89×10-4 at 635 K. NH4I(s)<-->NH3(g) + HI(g)...
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

  • The equilibrium constant, Kc, for the following reaction is 1.31×10-2 at 700 K. NH4I(s) (forward/reverse arrow)NH3(g)...

    The equilibrium constant, Kc, for the following reaction is 1.31×10-2 at 700 K. NH4I(s) (forward/reverse arrow)NH3(g) + HI(g) 1. Calculate Kc at this temperature for the following reaction: NH3(g) + HI(g) (forward/reverse arrow)NH4I(s) Kc = 2. The equilibrium constant, Kc, for the following reaction is 2.03 at 677 K. 2NH3(g) (forward/reverse arrow)N2(g) + 3H2(g) Calculate Kc at this temperature for: N2(g) + 3H2(g) (forward/reverse arrow)2NH3(g) Kc =

  • The equilibrium constant, Kc, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) <-->NH3(g) +...

    The equilibrium constant, Kc, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) <-->NH3(g) + HI(g) Calculate the equilibrium concentration of HI when 0.354 moles of NH4I(s) are introduced into a 1.00 L vessel at 673 K. [HI]= ____M

  • The equilibrium constant, K, for the following reaction is 9.25×10-3 at 692 K. NH4I(s) NH3(g) +...

    The equilibrium constant, K, for the following reaction is 9.25×10-3 at 692 K. NH4I(s) NH3(g) + HI(g) An equilibrium mixture in a 12.1 L container at 692 K contains 0.348 mol NH4I(s), 0.118 M NH3 and 7.84×10-2 M HI. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.98 L? [NH3] = M [HI] = M

  • The equilibrium constant, K, for the following reaction is 6.76×10-3 at 685 K. NH4I(s) NH3(g) +...

    The equilibrium constant, K, for the following reaction is 6.76×10-3 at 685 K. NH4I(s) NH3(g) + HI(g) An equilibrium mixture in a 11.7 L container at 685 K contains 0.229 mol NH4I(s), 0.101 M NH3 and 6.69×10-2 M HI. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 6.27 L?

  • The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s)----> NH3(g) +...

    The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s)----> NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.388 mol NH4I, 8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.46×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3]   = ______ M [HI]   = _______ M

  • The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) -->NH3(g) +...

    The equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH4I(s) -->NH3(g) + HI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 673 K contains 0.335 mol NH4I,   8.37×10-3 M NH3 and 8.37×10-3 M HI. If the concentration of NH3(g) is suddenly increased to 1.28×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?

  • -The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) +...

    -The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.452 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K. [HCl] = _________M -The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g) + I2(g)  2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.380 moles of H2and 0.380 moles of I2are introduced into a 1.00...

  • The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400...

    The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g)+ HI(g) NH4I(s) at 400 °C is 4.65. (a) If the partial pressure of ammonia is PNH, 0.881 atm and solid ammonium iodide is present, what is the equilibrium partial pressure of hydrogen iodide at 400 °C? PHI atm (b) An excess of solid NH,I is added to a container filled with NH3 at 400 °C and a pressure of 1.17 atm. Calculate the pressures of NH(g) and HI(g)...

  • a) The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g)...

    a) The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.318 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] = _____M b) The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.313 moles of COCl2(g) are introduced into a 1.00 L vessel...

  • The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g)...

    The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 5.41 L container at 548 K contains 1.17 mol of NH4Cl(s) and 0.350 mol of NH3, the number of moles of HCl present is ( ) moles. The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three...

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