Sulfur atoms combine to form molecules thathave different numbers of atoms dependingon the temperature. At about 1050°C, thefollowing dissociation occurs.Salg) = 4SziglThe initial concentration of Sag) in a flask is9.2 x 10³ mol/L, and the equilibrium concen-tration of the same gas is 2.3 x 10 mol/L.What is the value of K₂?

given reaction S8 (g) ⇌ 4 S2 (g) at equilibrium positionThe equilibrium constant (KC ) =…

Sulfur atoms combine to form molecules that have different numbers of atoms depending on the temperature. At about 1050°C, the following dissociation occurs. Salg 482) The initial concentration of Sai) in a flask is 9.2 x 10³ mol/L, and the equilibrium concen- tration of the same gas is 2.3 x 10 mol/L. What is the value of Ke?

Sulfur atoms combine to form molecules that have different numbers of atoms depending on the temperature. At about 1050°C, the following dissociation occurs. Salg 482) The initial concentration of Sai) in a flask is 9.2 x 10³ mol/L, and the equilibrium concen- tration of the same gas is 2.3 x 10 mol/L. What is the value of Ke?

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

When the reaction below is at equilibrium there are 0.250 mol of Br2, 1.25 mol of Cl2, and 1.5 mol of BrCl in a closed flask of 1.00 L at 100 degrees C. A Chem 109 student upsets the equilibrium by adding 0.0500 mol of Br2 into the 1L sealed flask. The equilibrium constant for the reaction is Kc = 7.20 at 100 degrees C. Calculate the concentration of Br2, Cl2 and BrCl when the new equilibrium is established. Br2 (g) + Cl2 (g) <---> 2 BrCl (g) Kc = 7.20 at 100 degrees C
Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(g) + 502(g) → 4 NO(g) + 6H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound pressure at equilibrium NH3 23.4 atm O2 40.2 atm NO 87.8 atm H,0 63.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
K, for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I½(g) = 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.315 M. [H2] = M [I] = M %3D [H国=
= KINETICS AND EQUILIBRIUM Setting up a reaction table Suppose a 500. mL flask is filled with 1.7 mol of N₂ and 0.10 mol of NH3. This reaction becomes possible: N₂(g) + 3H₂(g)2NH, (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 N₂. You can leave out the M symbol for molarity. initial change equilibrium N₂ 0 0 H₂ 0 0 0 NH3 0 0 00 1/5 X
Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
Carbon tetrachloride can be produced by the following reaction: CS2(g)+3 Cl2 (g)S, Cla (s) +CCL, (g) Suppose 1.20 mol of CS2 and 3.60 mol of Cl2 were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.61 mol of CC14. Calculate Kc at the unknown temperature.
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.
5. Phosphorus pentachloride gas, PCI,(g), will decompose to phosphorous trichloride, PCI,(g), and chlorine, Cl,(g), at 160 °C. In a sealed vessel, the reaction will proceed to equilibrium: PCI,(g) PCI, (g) + Cl(g) A chemist places 3.00 mol of phosphorous penta- chloride gas into a sealed 1.50 L flask at 160 °C. At equilibrium, he observes there is 0.300 mol of phosphorous trichloride gas and some chlorine gas. Calculate the equilibrium concentrations of gaseous phosphorous pentachloride and chlorine. m
An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) ⇒ CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂ I mol
2. 1.00 mol of oxygen and 1.00 mol of sulfur dioxide are placed into a 1.0-L flask. Sulfur trioxide gas is formed. At 1000 K, when equilibrium has been reached, 0.93 mgl pf sulfur trioxide have been formed. What is the Kec?.
Nitrosyl bromide decomposes to NO and Br2 in an endothermic process (A,H° = 16.3 kJ/mol-rxn). 2 NOBr(g) ⇒ 2 NO(g) + Br2 (g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. a. adding more NOBr(g) shift left shift right O no change b. adding more Br₂(g) shift left shift right O no change c. increasing the volume of the reaction flask shift left shift right O no change d. lowering the temperature shift left shift right O no change