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)
For the system: H2(g) + Cl2(g) ↔ 2HCl(g) ; ΔGo = -190.6 kJ at 25oC. Calculate...
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 =...
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
DH=DUIDIN 1. In following reaction H2(g) + Cl2(g) + 2HCl(g) AH=- 184.6 kJ/mol If 4 moles of H2 react with 4 moles of Cl, to form HCI. Calculate AU for this reaction, assumimg the reaction goes to completion against a pressure of 138.0 atm at constant volume. (IL atm = 101.3 J) pranai DU=q tw A) -738.4 kJ B) -369.2 kJ C) 138.0 kJ D) 184.6 kJ E) 244.5 kJ 4H =-92.3 ou-bH
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.
The reaction of hydrogen and chlorine gases produces hydrogen chloride. Cl2(g) + H2(g) → 2HCl(9) AHºrn =-184 kJ/mol Calculate the quantity of heat evolved if 180.g of chlorine reacted with 4.0 g of hydrogen. (a) (b) (c) (d) (e) -180 kJ 470 kJ 370 kJ 2.5 kJ 180 kJ
The value of ΔH° for the reaction below is-186 k. H2 (g) + Cl2 (g)-> 2HCl (g) The value of AHfo for HCI (g) is .k/ kJ/mol. O -3.72 x 102 ○-1.27 × 102 ○-93.0 0-186 ○ +186
For the reaction 2HBr(g) + Cl2(g)—>2HCl(g) + Brz(9) AH° = -81.1 kJ and AS° = -1.2 J/K The equilibrium constant for this reaction at 269.0 K is Assume that AHⓇ and AS are independent of temperature. Submit Answer Retry Entire Group 8 more group attempts remaining For the reaction N2(g) + 3H2(g) +2NH3(g) AH° = -92.2 kJ and A Sº = -198.7 JK The equilibrium constant for this reaction at 308.0 K is Assume that AHⓇ and AS are independent...
Suppose a 500.mL flask is filled with 0.60mol of H2 and 0.70mol
of Cl2. The following reaction becomes possible:
H2(g) + Cl2(g) 2HCl(g)
The equilibrium constant K for this reaction is 5.52 at the
temperature of the flask.
Calculate the equilibrium molarity of Cl2. Round your answer to
two decimal places.
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH =-184.6 kJ/mol If 5.0 moles of H2 reacts with 5.0 moles of C12 to form HC1 at 1.0 atm, what is Δ U for this reaction? Assume the reaction goes to completion and Δ V= 0 L (The conversion factor is 1 L·atm = 101.3 J.) kJ
For the reaction Fe(s) + 2HCl(aq) FeCl2(5) + H2(g) AH° = -7.4 kJ and AS° = 107.9 J/K The equilibrium constant for this reaction at 281.0 K is Assume that AHº and ASº are independent of temperature.