Equilibrium and Stoichiometry (two parts) A mixture of 0.186 mol of NOCI, 0.436 mol of NO and 0.520 mol of Cl, is allowed to reach equilibrium. 2NOCI(g) = 2NO(g) + Cl2(g) Suppose that, at equilibrium, it is found that 0.218 mol of NOCI is present. How many moles of Cl2 are present at equilibrium? (Answer to the nearest 0.001 mol and include the unit.)

Equilibrium and Stoichiometry (two parts) A mixture of 0.186 mol of NOCI, 0.436 mol of NO and 0.520 mol of Cl, is allowed to reach equilibrium. 2NOCI(g) = 2NO(g) + Cl2(g) Suppose that, at equilibrium, it is found that 0.218 mol of NOCI is present. How many moles of Cl2 are present at equilibrium? (Answer to the nearest 0.001 mol and include the unit.)

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

Pravinbhai
Suppose a 500. mL flask is filled with 1.3 mol of O, and 0.10 mol of SO3. This reaction becomes possible: 2s0,(g) +0,(g) – 2s0;(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 0,. You can leave out the M symbol for molarity. 2. so, 02 so, initial change equilibrium
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 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.
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 1.1 mol of CO, 1.9 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂ (g) + H₂ (g) The equilibrium constant K for this reaction is 4.24 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X S
Suppose a 250. mL flask is filled with 1.9 mol of O₂ and 1.7 mol of NO. The following reaction becomes possible: 2 N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 0.855 at the temperature of the flask. Calculate the equilibrium molarity of O₂. Round your answer to two decimal places. M Ś ?
3. (a) (b) (c) (d) Write the expression for the equilibrium constant (K) of the following reactions: Fe2+ (aq) + 2OH(aq) Fe(OH)₂ (s) CH4 (g) + 3 H2O (g) = CO (g) + 3 H₂ (g) 2 NO(g) + O₂(g) = 2 NO₂ (g) 2+ Zn(s) + Cu²+ (aq) = Zn²+ (aq) + Cu(s)
Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 0.30 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 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 H₂. You can leave out the M symbol for molarity. initial change equilibrium H₂ 0 X 0 1₂ 0 0 0 HI 0 0 0 010 X Ś
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 75 L tank with 22. mol of carbon monoxide gas and 26. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 13.5 mol of carbon monoxide gas, 17.5 mol of water vapor and 8.5 mol of hydrogen gas. The engineer then adds another 7.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. || mol x10