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 at 600 K.
| [COCl2] | = | ___M |
| [CO] | = | ___M |
| [Cl2] | = | ___M |
Homework Answers
Add Answer to:
a) The equilibrium constant, Kc, for the following
reaction is 1.80×10-4 at
298 K.
NH4HS(s)
NH3(g)...
The equilibrium constant, Kc, for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) H3(g) +H2S(g)...
The equilibrium constant, Kc, for the following
reaction is 1.80×10-4 at
298 K.
NH4HS(s) H3(g) +H2S(g) Calculate the equilibrium concentration of H2S when 0.261 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =
The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) goes to...
The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) goes to CO(g) + Cl2(g) . Calculate the equilibrium concentrations of reactant and products when 0.329 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COCl2] = ___M [CO] = ___M [Cl2] = -__M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) goes to COCl2(g) . Calculate the equilibrium concentrations of reactant and products when 0.320 moles of CO and 0.320 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = ___M [Cl2] = ___M [COCl2] = ___M
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) +...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.327 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = M [CH4] = M [CCl4] = M 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 0.275 moles of COCl2(g) are...
The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) ----> CO(g)...
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 0.362 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COCl2] = _____ M [CO] = _____ M [Cl2] = ____ M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.325 moles of CO and 0.325 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.355 moles of CO and 0.355 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
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...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PCl3(g) + Cl2(g) -----> PCl5(g) Calculate the equilibrium concentrations of reactant and products when 0.504 moles of PCl3 and 0.504 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = _____ M [Cl2] = _____M [PCl5] = _____M
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g)...
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g) -> 2 CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.251 moles ofCH4and 0.251 moles of CCl4are introduced into a 1.00 L vessel at 350 K. [ CH4] = M [ CCl4] = M [ CH2Cl2] = M b) The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) ->PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant...
The equilibrium constant, Kc, for the following
reaction is 1.80×10-4 at
298 K.
NH4HS(s) H3(g) +H2S(g) Calculate the equilibrium concentration of H2S when 0.261 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =
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