A 1.00-L flask is filled with 1.00 moles of H_2 and 2.00 motes of I_2. The...
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
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
4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO, and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, Kc. 5. (12 Pts) At a particular temperature, Kc = 1.00 x 10 for the reaction H2(g) + 12(g) = 2 HI(g) In an experiment,...
Suppose a 500. mL flask is filled with 2.0 mol of I_2 and 0.40 mol of HI. The following reaction becomes possible: H_2(g) + IK_2(g) 2HI(g) The equilibrium constant K for this reaction is 9.22 at the temperature of the flask. Calculate the equilibrium molarity if I_2.
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
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] =
K_c for the reaction of hydrogen and iodine to produce hydrogen iodide, H_2(g)+I_2(g) doubleheadarrow 2HI(g) is 54.3 at 430 degree C. Determine the initial and equilibrium concentration of H_2and I_2 are both 0.11 M and their equilibrium concentrations are both 0.048 M at 430 degree
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?
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...
For the following system, 0.400 moles of I_2, . 0.400 moles of Br_2 and 2.10 moles of IBr are placed in a 2.00- L flask. The value of K_c for the reaction is 110.25. What are the concentrations (M) of Br_2 and IBr (in this order) when equilibrium is reached? I_2(g) + Nr_2(g) 2 IBr(g) a) 0.116, 1.22 b) 0.109, 1.14 c) 0.100, 1.05 d) 0.013, 1.42 e)none of these