At a certain temperature, the reaction 2HF(g) H2(g) + F2(g) has Kc = 1.2 × 10-13. Does this reaction proceed far towards completion when equilibrium is reached? If 0.029 mol HF was placed in a 1.00 L container, and permitted to come to equilibrium, what would be the concentration of H2 and F2 in the container? Concentration of F2 at equilibrium = i M Concentration of H2 at equilibrium = i M

At a certain temperature, the reaction 2HF(g) H2(g) + F2(g) has Kc = 1.2 × 10-13. Does this reaction proceed far towards completion when equilibrium is reached? If 0.029 mol HF was placed in a 1.00 L container, and permitted to come to equilibrium, what would be the concentration of H2 and F2 in the container? Concentration of F2 at equilibrium = i M Concentration of H2 at equilibrium = i M

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

Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H₂, 8.0 M N₂, and 4.0 M NH 3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. N₂(g) + 3 H₂(g) = 2 NH3(g) Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2.0 0 2.0 5.0 -5.0 N₂(g) 8.0 1 6.0 + 4.0 -6.0 3 H₂(g) -4.0 10.0 2 NH3(g) RESET 11.0
Consider the equilibrium reaction: 2SO2(g) + O2(g)---->2SO3(g). You place 1.00 mol/L each of SO2 and O2 in a flask and find that at equilibrium the concentration of SO2 is 0.075 mol/L. What is the equilibrium constant for the reaction of SO2 and O2?
a. Suppose the reaction system CH4 (9) +202 (9) ⇒ CO2 (g) + 2H₂O(1) has already reached equilibrium. The position of the equilibrium was shifted by removing any liquid water from the system. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. O It will shift to the left. O It will not be affected. b. Suppose the reaction system CH4 (9) +202 (9) ⇒ CO2 (g) + 2H₂O(1) has already reached equilibrium. The position of the equilibrium was shifted by adding CO₂ to the system by dropping a chunk of dry ice into the reaction vessel. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. It will shift to the left. O It will not be affected. c. Suppose the reaction system CH4 (g) +20₂ (9) — CO2 (g) + 2H₂O(1) has already reached equilibrium. The position of the equilibrium was shifted by performing the…
Suppose a 500. mL flask is filled with 0.20 mol of Br,, 1.6 mol of OCl, and 1.9 mol of BrOCl. The following reaction becomes possible: 2' Br, (g) +OCl, (g)- BROCI(g)+BrC1(g) The equilibrium constantK for this reaction is 5.57 at the temperature of the flask. Calculate the equilibrium molarity of BrOCl. Round your answer to two decimal places. O M
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
In a particular experiment, it was found that when O2(g) and CO(g) were mixed and allowed to react according to the equation 2C0(g) + O2(g) 2CO2(g) the O2 concentration had decreased by 0.036 molL1when the reaction reached equilibrium. How had the concentrations of CO and CO2 changed? Incorrect. [CO] decrease = i ! mol/L Incorrect. [CO2] increase = i mol/L
Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 1.54x10-3 moles of NH3(g), 0.549 moles of N₂, and 0.352 moles of H₂ are at equilibrium in a 19.7 L container at 792 K, the value of the equilibrium constant, K, is
Suppose a 250. mL flask is filled with 0.30 mol of NO and 0.80 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g)<->2NO2(g) The equilibrium constant K for this reaction is 0.717 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?
For the equilibrium, 2NO(g)+2H₂(g)→→N₂(g)+2H₂O(g), what will happen if it were in a rigid vessel and argon gas (Ar) were added to the system? Assume temperature remains constant. there will be no change in the equilibrium O the equilibrium will shift toward reactants the equilibrium will be pushed forward there will be a change in the value of the equilibrium constant
Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(2)- -2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 O2 NO initial change equilibrium olo
At a certain temperature, the reaction 2HF(g) a H2(3) + F2(g) has K = 1.2 x 10-13. Does this reaction proceed far towards completion when equilibrium is reached? If 0.022 mol HF was placed in a 1.00 L container, and permitted to come to equilibrium, what would be the concentration of H2 and F2 in the container? Concentration of F2 at equilibrium = i M Concentration of H2 at equilibrium = i M