-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 L vessel
at 698 K.
[ H2] | = | _______M |
[ I2] | = | _______M |
[ HI ] | = | _______M |
THANK YOU
-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 55.6 at 698 K. H2 (g) + I2 (g) ---> 2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.301 moles of H2 and 0.301 moles of I2 are introduced into a 1.00 L vessel at 698 K. [ H2 ] = _______ M [ I2 ] = ________ M [ HI ] = _______ M
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 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.293 moles of H2 and 0.293 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M [I2] = M [HI] = M
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.276 moles of H2 and 0.276 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = _____M [I2] =______M [HI] =______M
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 0.249 moles of PCl3 and 0.249 moles of Cl2 are introduced into a 1.00 L vessel at 500 K. [PCl3] = M [Cl2] = M [PCl5] = M The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) = H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2 (g) + 12 (g) = 2 HI(g) Calculate the equilibrium concentrations of reactants and product when 0.286 moles of H2 and 0.286 moles of 12 are introduced into a 1.00 L vessel at 698 K. M [H2) = [12] = [HI]= M M Submit Answer Retry Entire Group 9 more group attempts remaining
The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at698 K.2HI(g) → H2(g) + I2(g)Calculate the equilibrium concentrations of reactant and products when 0.223 moles of HI are introduced into a 1.00 L vessel at 698 K.[HI]= ?[H2]= ?[I2]= ?
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K. PC13(g) + Cl2(g) = PC15(g) Calculate the equilibrium concentrations of reactant and products when 0.389 moles of PC13 and 0.389 moles of Cl2 are introduced into a 1.00 L vessel at 500 K [PC13] = [Cl] = [PC15] - The equilibrium constant, Kc, for the following reaction is 5.10x10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.467 moles of NHACI(S)...
1- The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) --------> H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.395 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] = M [H2] = M [I2] = M 2- student ran the following reaction in the laboratory at 1090 K: 2SO3(g) ----------> 2SO2(g) + O2(g) When he introduced SO3(g) at a pressure of 1.05 atm into a 1.00...
The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) ---------->2HI(g) 1) Calculate the equilibrium concentrations of reactants and product when 0.309 moles of H2 and 0.309 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] = M? [I2] = M? [HI] = M? 2.The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K: PCl5(g)------->PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a...