IV Consider the reaction: H_2 (g) + I_2 (g) = 2 HI(g) A reaction mixture in...
Consider the following reaction: H_2 (g) + I_2 (g) Equilibrium 2 HI (g) Complete the following table. Assume that all concentrations are equilibrium concentrations in M. Part A Find K_c at 25 degree C. Express your answer using three significant figures. K_c = _______ Part B Find [H_2] at 340 degree C. Express your answer using two significant figures. [H_2] = _______ M Part C Find [HI] at 445 degree C. Express your answer using three significant figures. [HI] =...
At 400 K, an equilibrium mixture of H_2, I_2, and HI consists of 0.068 mol H_2, 0.075 mol I_2, and 0.13 mol HI in a1.00-L flask. What is the value of K_p, for the flowing equilibrium? (R = 0.0821 L middot atm (K - mol)) 2HI_(g) Rightwardsharpoonoverleftwardsharpoon H_2 (g) + I_2 (g) A) 0.039 B) 3.4 C) 26 D) 0.29 E) 8.2 If K = 0.150 for A_2 + 2B Rightwardsharpoonoverleftwardsharpoon 2AB, what is the value of K for the...
The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K: H_2(g) + I_2(g) 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.351 moles of H_2 and 0.351 moles of I_2 are introduced into a 1.00 L vessel at 698 K. [H_2] = M [I_2] = M [HI] = M
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2 (g) + I_2 (g) 2HI (g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of HI if initial concentrations of H_2 and I_2 are both 0.10 M and their equilibrium concentrations are both 0.043 M at 430 degree C. [HI]_i = M [HI]_e = M
During an experiment, 0.986 mol H_2 and 0.493 mol I_2 were placed in a 1.95 L vessel where the following reaction came to equilibrium. H_2 (g) + I_2 (g) 2HI(g) For this reaction K_c = 49.5 at the temperature of the experiment. a) What were the equilibrium concentrations of H_2, I_2, and HI? [H_2] = [I_2] = [HI] =
Given the reaction 2HI(g) H_2(g) + I_2(g) K_eq = 1.0 times 10^1 A sample mixture of H1, H2, and I_2 at equilibrium, was found to have [H_2] = 3.6 times 10^-4 M and |HI] = 7.0 times 10^-2 M. Calculate the molar concentration of I_2 in the equilibrium mixture. [I_2] = M
At a particular temperature, K = 1.00 Times 10^2 for the following reaction. H_2(g) + I_2(g) 2 HI(g) IN an experiment, 1.39 mol H_2, 1.39 mol HI are introduced intoa 1.00-L, container, Calculate the concentrations of all species when equilibrium is reached. H_2 M I_2 M HI M
Consider the following reaction at 600K: A reaction mixture at equilibrium at 600K contains 0.170 bar H_2, 0.120 bar I_2 and 1.26 bar HI. Calculate the equilibrium constant (K_p) for this reaction A second reaction mixture, also at 600 K contains 0.135 bar of H_2, 0.135 bar I_2 and 1.10 bar of HI. Is the mixture at equilibrium? If the mixture in part b is not at equilibrium, what will be the partial pressures of H_2, I_2 and HI when...
The equation for the formation of hydrogen iodide from H_2 and l_2 is: H_2(g) + I_2(g) 2 HI(g) The value of K_p for the reaction is 69.0 at 790.0 degree C. What is the equilibrium partial pressure of HI in sealed reaction vessel at 790.0 degree C if the initial partial pressures of H_2 and l_2 are both 0.1800 atm an initially there is no HI present?
Consider this reaction: H 2 (g)+ I 2 (g)⇌2HI(g) H2(g)+I2(g)⇌2HI(g) A rxn mixture in a 3.73 L flask at a certain temperature initially contains 0.766 g H2 and 96.7 g I 2 I2 . At equilibrium, the flask holds 90.3 g HI . Calculate the equilibrium constant (Kc)(Kc) for the reaction at this temperature. Record your answer using two significant figures.