(12) 3. The reaction for the formation gaseous hydrogen fluoride from hydrogen and fluorine H2(g) + F2(g) 2 HF(g) has an equilibrium constant of 121 at a certain temperature. In a particular experiment, 3.00 moles of each component (H2, F2 and HF) were added to a 1.500 L flask. Calculate the concentrations of all species after equilibrium has been reached.

(12) 3. The reaction for the formation gaseous hydrogen fluoride from hydrogen and fluorine H2(g) + F2(g) 2 HF(g) has an equilibrium constant of 121 at a certain temperature. In a particular experiment, 3.00 moles of each component (H2, F2 and HF) were added to a 1.500 L flask. Calculate the concentrations of all species after equilibrium has been reached.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The equilibrium constant, Kc, for the following reaction is 0.0129 at 600 K. COC12 (g) CO(g) + Cl₂ (g) If an equilibrium mixture of the three gases in a 16.3 L container at 600 K contains 0.497 mol of COC1₂(g) and 0.339 mol of CO, the equilibrium concentration of Cl2 is || M.
The equilibrium constant, Kc, for the following reaction is 1.39 at 663 K. 2NH3 (9) N2(g) + 3H₂(g) When a sufficiently large sample of NH3(g) is introduced into an evacuated vessel at 663 K, the equilibrium concentration of H₂(g) is found to be 0.957 M. Calculate the concentration of NH3 in the equilibrium mixture. [NH3] = = M
Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium. The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M. CH4(g) + 2H2S(g) ↔ CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.
A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.
The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M
In a particular experiment, it was found that when O,(g) and CO(g) were mixed and allowed to react according to the equation 2Co(g) + O2(3) = 2CO2(3) the O2 concentration had decreased by 0.062 mol Lwhen the reaction reached equilibrium. How had the concentrations of CO and CO2 changed? [CO] decrease = i mol/L [CO2] increase = mol/L
A2
In an experiment, gaseous C2H4 and H2O, at 25 mmol each, were mixed in a 50-mL flask that contains 2.5 mmol of C2H6. (a) Determine the equilibrium constant if, at equilibrium, 16 mmol of C2H6 was present. C2H4(g) + H2O(g) ⇋ C2H6(g) + O2(g) At one point of the experiment, it was found that 9.7 mmol C2H4, 7.5 mmol H2O, 21.9 mmol C2H6 and 16.4 mmol O2 were present in the flask. (b) At what direction should the reaction proceed to achieve equilibrium? Support your answer with calculations and explain your answer in not more than 3 sentences.
3.2
Consider the following reaction: H2 (9) + 12 (9) = 2 HI (g) A reaction mixture in a 3.68 L flask at a certain temperature initially contains 0.764 g Hz and 97.1g Iz. At equilibrium, the flask contains 90.6 g HI. Part A Calculate the equilibrium constant (Ke) for the reaction at this temperature. Express your answer using two significant figures. ? K. = Submit RequestAnswer
Consider the following reaction: 2HI(g) → H₂(g) + 1₂ (9) If 2.74 moles of HI(g), 0.333 moles of H₂, and 0.588 moles of I2 are at equilibrium in a 10.3 L container at 878 K, the value of the equilibrium constant, Кси is
Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 0.0290 at 1150 K. 2SO3 (g)2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 19.7 L container at 1150 K contains 0.251 mol of SO3(g) and 0.353 mol of SO2, the equilibrium concentration of O₂ is M. Submit Answer Retry Entire Group 9 more group attempts remaining