If a reaction with equilibrium constant, K1, is subtracted from a reaction with equilibrium constant, K2, then the equilibrium constant for the resulting reaction, K3, is
A. K2 - K1
B. K2 * K1
C. K2 / K1
D. K1 / K2
E. different from any combination given here
If a reaction with equilibrium constant, K1, is subtracted from a reaction with equilibrium constant, K2,...
Learning Goal: To understand how to calculate the equilibrium constants for chemical equations that can be produced by the addition of other chemical equations with known equilibrium constants. For a chemical reaction equation with the general form aA+bB⇌cC+dD the equilibrium equation is given by K1=[C]c[D]d[A]a[B]b Thus, for a chemical reaction equation with the general form cC+dD⇌eE+fF the equilibrium equation is given by K2=[E]e[F]f[C]c[D]d If the first two equations are added together such that aA+bB⇌eE+fF then the equilibrium equation is given...
For the reaction mechanism ki A> В В -> А k2 A>С k3 |В >D sketch a graph showing how the concentrations of A,B,C and D change over time. Consider the following cases 1) k1>k-1 and k2>>k3>>k1 2) k1k-1 and k1>>k2= k3
For the reaction mechanism ki A> В В -> А k2 A>С k3 |В >D sketch a graph showing how the concentrations of A,B,C and D change over time. Consider the following cases 1) k1>k-1 and k2>>k3>>k1 2)...
Given that K1 and K2 are the respective equilibrium constants for the two reactions CO2(g) + H2(g) = CO(g) + H2O(l) K1 = 3.08×10-4 CdO(s) + H2(g) = Cd(s) + H2O(l) K2 = 40.7 Determine the equilibrium constant for the reaction CO(g) + CdO(s) = CO2(g) + Cd(s) K =
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+
Part ADetermine the value of the equilibrium constant, Kgoal , for the reactionN2(g)+O2(g)+H2(g)⇌12N2H4(g)+NO2(g) , Kgoal=?by making use of the following information:1. N2(g)+O2(g)⇌2NO(g) , K1 =4.10×10−312. N2(g)+2H2(g)⇌N2H4(g) , K2 =7.40×10−263. 2NO(g)+O2(g)⇌2NO2(g) , K3 =6.00×10−13Express your answer numerically.Part BDetermine the equilibrium constant, Kgoal , for the reaction4PCl5(g)⇌P4(s)+10Cl2(g), Kgoal=?by making use of the following information:P4(s)+6Cl2(g)⇌4PCl3(g), K1=2.00×1019PCl5(g)⇌PCl3(g)+Cl2(g), K2=1.13×10−2Express your answer numerically.
For a parallel reaction A goes to B with rate constant k1 and A goes to C with rate constant k2, you determine that the activation energies are 38.3 kJ/mol for k1 and 169.3 kJ/mol for k2. If the rate constants are equal at a temperature of 316 K, at what temperature (in K) will k1/k2 = 2?
Question 2 of 3 Two reactions and their equilibrium constants are given. A+2B 2C K1 2.77 2C D K2 0.198 Calculate the value of the equilibrium constant for the reaction D A + 2 B. K =
If the equilibrium constant for reaction X is K. What is the equilibrium constant for reaction Y is? Reaction X: SO2 (g) + (1/2) O2 (g) ⇌ SO3 (g) Reaction Y: 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) a. 2K b. K2 c. 1/K2 d. 0.5 x K e. -K2
Two reactions and their equilibrium constants are given. 33 A + 2B20 2C=D K1 = 2.09 K2 = 0.170 Calculate the value of the equilibrium constant for the reaction D = A + 2B. K=
Determine the value of the equilibrium constant, for the reaction CO2 (g) ⇌ C (s) + O2 (g), K = ? by making use of the following information: 2 CO2 (g) + 2 H2O (l) ⇌ CH3COOH (l) + 2 O2 (g), K1 = 5.00 2 H2 (g) + O2 (g) ⇌ 2 H2O (l), K2 = 100.0 CH3COOH (l) ⇌ 2 C(s) + 2 H2 (g) + O2 (g), K3 = 2.00