Consider the following reaction: 2HF(g) rightleftharpoons H_2(g) + F_2(g) (K_c = 1.00 times 10^-2) Given that...
The equilibrium constant K_c for the reaction H_2 (g) + Br_2(g) 2 HBr(g) is 2.180 times 10^6 at 730 degree C. Starting with 2.20 moles of HBr in a 21.6-L reaction vessel, calculate the concentrations of H_2, Br_2 and HBr at equilibrium. [H_2] = [Br_2] = [HBr] =
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
IV
Consider the reaction: H_2 (g) + I_2 (g) = 2 HI(g) A reaction mixture in a 4.25 L flask at a certain temperature initially contains 0.668 g H_2 (g) and 86.9 g of I_2 (g). At equilibrium, the flask contains 78.4 g HI. Calculate K_c degree for this reaction at this temperature.
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
Consider the following reaction where K_c = 77.5 at 600 K. CO(g) + Cl_2(g) COCl_2(g) A reaction mixture was found to contain 2.42 times 10^-2 moles of CO(g), 4.19 times 10^-2 moles of Cl_2(g) and 0.121 moles of COCl_2(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q_c, equals The reaction must run in the forward direction to reach equilibrium. must run 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] =...
2. Hydrogen fluoride can be produced from elemental fluorine and hydrogen according to the reaction H2(g) + F2(g) → 2HF(g). The reaction has an equilibrium constant, Kc, of 7.75 x 102 at a certain temperature. a. Calculate the equilibrium concentration of HF(g) if 5.750 mol of H, and Fz are introduced into a 1.500 L flask. b. Calculate the reaction quotient if 3.25 mol of EACH species is introduced into a 3.000 L flask. What does this value tell us...
The following reaction 2H_2S(g) 2H_2(g) + S_2(g), K_c = 1.67 times 10^-7 at 800degreeC is carried out at the same temperature with the following initial concentrations: [H_2S] = 0.100M, [H_2] = 0.100M, and [S_2] = 0.00 M. Find the equilibrium concentration of S_2. Express the molarity to three significant figures.
Consider the following reaction, 2AB (g) ⇌ A2 (g) + B2 (g) K = 1.50x10−2 At some point in the reaction, Q = 5.30. Which of the following statements is correct concerning the equilibrium? 0.60 mol of Br2 and 0.60 mol of Cl2 are placed in a 1.00 L flask and allowed to reach equilibrium. After reaching equilibrium, the flask is found to contain 0.28 mol of BrCl. What is the value of Kc for this reaction? Br2 (g) + Cl2 (g)...
Consider the following reaction between carbon monoxide and hydrogen, CO(g) + 2 H_2(g) Equilibrium CH_3OH(l) K_p = 2.25 times 10^4 Give the K_p expression for this reaction Determine the equilibrium pressure of CO if the P(H_2) at equilibrium = 0.52 atm If the Q_p for a particular reaction mixture was measure as 2.30 times 10^-4, how will this reaction proceed?