Suppose a 250. mL flask is filled with 0.80 mol of SO, and 1.5 mol of SO3. This reaction becomes possible: 2s0, (g) +0,(g) = 2Sso;(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 O2. You can leave out the M symbol for molarity. so2 O, so, initial change equilibrium

Suppose a 250. mL flask is filled with 0.80 mol of SO, and 1.5 mol of SO3. This reaction becomes possible: 2s0, (g) +0,(g) = 2Sso;(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 O2. You can leave out the M symbol for molarity. so2 O, so, initial change equilibrium

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

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
For the equilibrium 3NO2(g) K=1.0 × 10-11 N₂O5(g) + NO(g) If a 4.00 L container initially holds 0.23 mol of NO₂, how many moles of N₂O5 will be present when this system reaches equilibrium? Enter your answer in scientific notation. moles of N₂O5 = i x 10 i mol
Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.30 mol of H,O and 1.3 mol of H,. The following reaction becomes possible: CO(g) +H,0(g)– CO2(g)+H,(g) The equilibrium constant K for this reaction is 1.25 at the temperature of the flask. Calculate the equilibrium molarity of H,O. Round your answer to two decimal places. OM
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
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
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.
Write the equilibrium expression (Ke) for the reaction: PC1s(g) PC13(8) + C12(g)
Suppose a 250. mL flask is filled with 2.0 mol of Cl₂ and 1.2 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl (g) The equilibrium constant K for this reaction is 3.70 at the temperature of the flask. Calculate the equilibrium molarity of C12. Round your answer to two decimal places. Шм 000 Ar
Suppose a 500. mL flask is filled with 1.9 mol of N, and 0.20 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 3.27 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.8 mol of O2 and 0.30 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 2.61 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places. M X S
Suppose a 250. ml. flask is filled with 0.20 mol of O, and 2.0 mol of NO. The following reaction becomes possible: N2 (2) + 0, (g) - 2NO() The equilibrium constant K for this reaction is 8.08 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. OM
Suppose a 500. mL flask is filled with 0.20 mol of NO, and 1.3 mol of NO. This reaction becomes possible: 2NO,(g) = 2NO(g)+0,(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 O,. You can leave out the M symbol for molarity. NO, NO 0, initial ? change equilibrium