Balanced chemical reaction;
CH3Br + H2S --------> CH3SH + HBr
Kc = [CH3SH][HBr] / [CH3Br][H2S]
We can find Kc if we know the equilibrium concentrations of species.
what is the equilibrium constant of CH3Br + H2S H CH3SH + HBr and how to...
the value on top is -2.1kj/mol
2.1 kJ/mol. The following reaction has a value of AGⓇ = CH3Br + H2S CH,SH HBr a) Calculate key at room temperature (25°C) for this reaction as written. b) Starting with 1 M solution each of CH3Br and H2S, calculate the final concentration of all four species at equilibrium. Please be thorough in your presentation AGⓇ = -2.303RT(log kea); at 25°C, RT= 2478 J/mol or 2.48 kJ/mol
Calculate the partial pressure (in atm) of HBr at equilibrium when 3.16 atm of CH3Br and 6.55 atm of H2O react at 1000 K according to the following chemical equation: CH3Br (g) + H2O (g) ⇌ CH3OH (g) + HBr (g) Kp = 6.66×10-2 Report your answer to three significant figures in scientific notation.
Methanol (CH3OH) is converted to Bromomethane (CH3Br) as follows: CH3OH +HBr= CH3Br+H2O If 8.01 g of Bromomethane are produced when 4.051 g of methanol is reacted with excess HBr, what is the percentage yield?
Methanol (CH3OH) is converted to bromomethane (CH3BR) as follows: CH3OH + HBr → CH3B + H2 (balanced) If 7.00 g of bromomethane (CH3Br) are produced when 2.42 g of methanol (CH3OH) is reacted with excess HBr, what is the percentage yield?
Given the two reactions H2S(aq)⇌HS−(aq)+H+(aq), K1 = 9.62×10−8, and HS−(aq)⇌S2−(aq)+H+(aq), K2 = 1.42×10−19, what is the equilibrium constant Kfinal for the following reaction? S2−(aq)+2H+(aq)⇌H2S(aq)
Given the two reactions H2S⇌HS−+H+, K1 = 9.03×10−8, and HS−⇌S2−+H+, K2 = 1.10×10−19, What is the equilibrium constant Kfinal for the following reaction? S2−+2H+⇌H2S
Given the two reactions H2S⇌HS−+H+, K1 = 9.64×10−8, and HS−⇌S2−+H+, K2 = 1.49×10−19, what is the equilibrium constant Kfinal for the following reaction? S2−+2H+⇌H2S
Part A= Given the two reactions H2S⇌HS−+H+, K1 = 9.42×10−8, and HS−⇌S2−+H+, K2 = 1.32×10−19, what is the equilibrium constant K final for the following reaction? S2−+2H+⇌H2S Part B= Given the two reactions PbCl2⇌Pb2++2Cl−, K3 = 1.89×10−10, and AgCl⇌Ag++Cl−, K4 = 1.23×10−4, what is the equilibrium constant K final for the following reaction? PbCl2+2Ag+⇌2AgCl+Pb2+
At 298K, the equilibrium constant for the following reaction is 1.00 107 H2S(aq) + H2O- H30"(aq) + HS-(aq) The equilibrium constant for a second reaction is 1.00 10-19. Use this information to determine the equilibrium constant for the reaction: (aq)+2H2O 2H3O K- Submit Answer Retry Entire Group 9 more group attempts remaining
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] =