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 =
If the reaction is reversed the new equilibrium constant becomes inverse of the original one.
Kc' = 1/Kc
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 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=?
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
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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) + 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?
Question The equilibrium constant, Kc, for the following reaction is 3.72 at 701 K. 2NH3(gN2(g) + 3H2(g) Calculate Kc at this temperature for the following reaction: 1/2N2(g) +3/2H2(g) NH3( Kc
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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...