Write the equilibrium constant expression : CH4 (g) + Cl2 (g) = CH3Cl (g) + HCl (g)
Write the equilibrium constant expression : CH4 (g) + Cl2 (g) = CH3Cl (g) + HCl...
Chloromethane forms by the reaction CH4(g) + Cl2(g) ⇌ CH3Cl(g) + HCl(g) at 1500K, Kp = 1.6 x 104 . In the reaction mixture, PCH4 = 0.13 atm, PCl2 = 0.035 atm, PCH3Cl = 0.24 atm, and PHCl = 0.47 atm. Is CH3Cl or CH4 forming?
A-The following reaction has a Kp=1.6 x 104 at 1500 K. CH4(g) + Cl2(g) CH3Cl(g) + HCl(g) a. In a reaction mixture, PCH4 = 0.13atm , PCl2 = 0.035atm , PCH3Cl = 0.24atm , and PHCl = 0.47atm . Is the system at equilibrium? If not how does the reaction proceed to reach equilibrium? At equilibrium, the following stresses are applied. How is the equilibrium affected? Explain. i. HCl is removed. ii. CH3Cl is added iii. The volume is reduced...
Write an expression for the equilibrium constant of each chemical equation. SbCl5(g)⇌SbCl3(g)+Cl2(g)SbCl5(g)⇌SbCl3(g)+Cl2(g) 2 BrNO (g)⇌2 NO(g)+Br2(g)2 BrNO (g)⇌2 NO(g)+Br2(g) CH4(g)+2 H2S(g)⇌CS2(g)+4 H2(g)CH4(g)+2 H2S(g)⇌CS2(g)+4 H2(g) 2 CO(g)+O2(g)⇌2 CO2(g)
When 20.5 g CH4 (MM = 16.04 g/mol) and excess Cl2 undergo a reaction that has a 90.5% yield, what mass of chloromethane (CH3Cl, MM = 50.48 g/mol) forms? CH4(g) + Cl2(g) --> CH3Cl(g) + HCl(g)
Write the pressure equilibrium constant expression for this reaction. .NH,Cl(s)— NH3(g)+HCl(9) x 5 ?
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...
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
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 =...
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations: C(s)+H2(g)-->CH4 H= -74.6 kJ C(s) + Cl2(g)--> CCl4 H=-95.7 kJ H2(g)+Cl2(g)--> HCl H=-92.3 kJ
The equilibrium constant expression K p for the reaction CH4 (g) +2O2 (g) <--> CO2 (g) + 2H2O (g) is __________. A. Kp = PCO2PH2O 2/PCH4PO22 B. Kp = PCH4PO22/PCO2PH2O 2 C. Kp = PCH4PO2/PCO2PH2O D. Kp = PCO2PH2O /PCH4PO2