H2(g) + Cl2(g) ↔ 2 HCl(g) If the initial concentration of HCl is 0.263 M and...
H2(g) + Cl2(g) ↔ 2 HCl(g) If the initial concentration of HCl is 0.263 M and the equilibrium constant Kc = 0.381, what is the Cl2 concentration at equilibrium? Answer to 3 decimal places and be sure to include your units.
Use the equilibrium below to answer the following questions. H2(g) + Cl2(g) ↔ 2 HCl(g) If the initial concentration of HCl is 0.151 M and the equilibrium constant Kc = 0.287, what is the HCl concentration at equilibrium? Answer to 3 decimal places and be sure to include your units. Use the equilibrium below to answer the following questions. H2(g) + Cl2(g) ↔ 2 HCl(g) If the initial concentration of HCl is 0.151 M and the equilibrium constant Kc =...
Use the equilibrium below to answer the following questions. H2(g) + Cl2(g) # 2 HCl(g) If the initial concentration of HCl is 0.378 M and the equilibrium constant Kc = 0.223, what is the Cl2 concentration at equilibrium? Answer to 3 decimal places and be sure to include your units. Answer: Use the equilibrium below to answer the following questions. H2(g) + Cl2(g) # 2 HCl(g) If the initial concentration of HCI is 0.378 M and the equilibrium constant Kc...
Br2 (g) + Cl2 (g) ↔ 2 BrCl (g) A reaction mixture at equilibrium contains [Br2] = 0.0993 M, [Cl2] = 0.0967 M, and [BrCl] = 0.0285 M. Calculate the equilibrium constant Kc.
Consider the reaction: PCl5 (g) ⇔ PCl3 (g) + Cl2 (g) The initial concentration of PCl5 is 0.40 M and the equilibrium concentration of PCl3 is 0.33 M. Calculate the equilibrium constant Kc.
For the system: H2(g) + Cl2(g) ↔ 2HCl(g) ; ΔGo = -190.6 kJ at 25oC. Calculate the equilibrium constant. (be careful of the negative sign)
The following reaction, in CCl4 solvent, has been studied at 25°C. 2BrCl ↔ Br2 + Cl2 The equilibrium constant Kc is known to be 5.0x10-5. If the initial concentration of chlorine is 0.027 M and of bromine monochloride is 0.061 M, what is the equilibrium concentration of bromine?
The equilibrium constant Kc for the following reaction is 8.30. H2(g) + CO2(g) ↔ H2O(g) + CO(g) Initially, 0.40 moles each of H2 and CO2 are injected into a 9.00 L flask. Calculate the concentration of the CO(g) at equilibrium.
For the reaction H2(g) +
Cl2(g) 2 HCl(g), the
equilibrium constant K at 800oC is 4.35 x
104.
Hydrogen and chlorine, each at a partial pressure of 0.700 bar,
are placed in a vessel at 800oC and allowed to
equilibrate. Find the final partial pressures of all three gases in
this reaction.
p(H2) = bar
p(Cl2) =
. bar
p(HCl) =
bar
Consider the reaction: SO2Cl2(g) SO2(g) + Cl2(g) A reaction mixture contains an initial concentration of [SO2Cl2] = 0.020M. At equilibrium, [Cl2] = 1.2 x 10-2 M. Calculate the value of Kc.