Suppose a 250. mL flask is filled with 0.60 mol of SO₂ and 1.0 mol of SO3. This reaction becomes possible:2SO₂(g) + O₂(g) — 2SO3(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 theequilibrium molarity of each compound after the reaction has come to equilibrium.Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity.initialchangeequilibriumSO₂0₂0X0SO₂0010XŚ

Since, Molarity is the number of moles of solute dissolve in one litre of the solution. Thus,

Suppose a 250. mL flask is filled with 0.60 mol of SO₂ and 1.0 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g)2SO3(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 equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. initial change equilibrium SO₂ 0 0 0₂ 0 X 0 SO3 0 U 0

Suppose a 250. mL flask is filled with 0.60 mol of SO₂ and 1.0 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g)2SO3(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 equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. initial change equilibrium SO₂ 0 0 0₂ 0 X 0 SO3 0 U 0

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

Suppose a 250. mL flask is filled with 0.90 mol of CO, 0.50 mol Of NO and 0.80 mol of CO ₂. The following reaction becomes possible: NO₂(g) + CO (g) → NO(g) + CO₂(g) The equilibrium constant x for this reaction is 0.980 at the temperature of the flask. Calculate the equilibrium molarity of No. Round your answer to two decimal places. ? olo 18 Ar
Suppose a 500. mL flask is filled with 1.4 mol of N2 and 0.70 mol of NO. This reaction becomes possible: N2(g) + O2(g) = 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 r to stand for the unknown change in the molarity of N2. You can leave out the M symbol for molarity.
Setting up a reaction table Suppose a 500. mL flask is filled with 0.10 mol of H₂ and 0.60 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound 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 H₂. You can leave out the M symbol for molarity. [H₂] [42] initial change equilibrium x [HI]
For the equilibrium reaction 2SO 2(g) + O 2(g) <-> 2SO 3(g), ΔHº rxn = –198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase? Add SO2 gas. Add a catalyst. None of these. Decrease the temperature. Remove O2 gas.
Suppose a 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.54 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M Images X
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 125 L tank with 45. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 12. mol of nitrogen dioxide gas. The engineer then adds another 11. mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. | mol x10
Pravinbhai
Suppose a 500. mL flask is filled with 1.7 mol of CO, 0.50 mol of CO2 and 0.90 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 1.14 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś
The following reaction is investigated: Initially there are 0.44 mol of N20 and 0.45 mol of N2H4 in a container. If the amount of N2 at equilibrium is 0.174 mol, how many moles of N20 are present at equilibrium? 2N20 (g) + N2H4 (g) 5 3N2 (g) + 2H2O (g) Report your answer as a decimal with two significant figures.
Suppose a 500. mL flask is filled with 0.70 mol of NO2, 1.7 mol of CO and 0.30 mol of NO. The following reaction becomes possible: NO₂(g) + CO (g) → NO(g) + CO₂(g) The equilibrium constant K for this reaction is 8.94 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ☐M X Ś
Suppose a 250. mL flask is filled with 1.2 mol of NO and 0.90 mol of NO 2. The following reaction becomes possible: NO3(g) + NO(g) = 2NO2(g) The equilibrium constant K for this reaction is 0.661 at the temperature of the flask. Calculate the equilibrium molarity of NO 3. Round your answer to two decimal places. Ом ☑
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "Nox") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 75 L tank with 23. mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 17.9 mol of nitrogen dioxide gas. The engineer then adds another 7.7 mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.