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

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

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

What happens to an endothermic reaction when an equilibrium system is heated? The system shifts forward. The system shifts backward. The equilibrium does not shift to maximize the stress. or The equilibrium does not shift to restore original conditions.
Keq from Equilibrium Composition, Variously Expressed. At some temperature, an equilibrium mixture, in a 1.00-L container, involving the chemical system PCI5(g) = PCI3(g) + Cl2(g) is found to contain 5.74×1020 molecules of PCI5, 0.00921 mol of PCI3, and 0.228 g of Cl2. Calculate the equilibrium constant (Keg expressed in terms of the molar concentrations) at this temperature. (No units required.)
Sulfur trioxide gas can be converted into sulfur dioxide gas according to the following equation: 2 SO2 ) 2 SO3 (2) O2 (g) Initially, 0.568 mol of sulfur trioxide was placed in a 2.00L container. When the system was allowed to reach equilibrium, it was determined that 0.185 mol/L of sulfur dioxide was present. Calculate the value of Keg for this reaction.
3. For a gas-phase equilibrium reaction you are studying, Kc Kp. Which side of the reaction is favored in the equilibrium? Which side of the reaction has a larger number of gas molecules?
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.
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75 L tank with 10. mol of ethylene gas and 5.4 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.8 mol of ethylene gas and 2.2 mol of water vapor. The engineer then adds another 1.4 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. |mol x10 O
Hydrogen lodide is produced by combining hydrogen gas and iodine gas as shown in the balanced chemical reaction below. If H2 and 12 each have an Initial pressure of 1.73 atm, what is the equilibrium pressure of HI? The equilibrium constant for the reaction is 137. H2 (9) + 12 (9) = 2HI (g) Report your answer to two decimal places. Do not put a unit. A Moving to another question will save this response. Question 12 of 30
"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 18. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.0 mol of carbon monoxide gas, 12. mol of water vapor and 12. mol of carbon dioxide. The engineer then adds another 9.0 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. Answer Submitted: mol M 00
Pravinbhai
Consider the following reaction: 2 NO + Cle = 2 NOCI K = 2.13 x 103 Which compound(s) will be present in the greatest amount once this reaction reaches equilibrium? Explain.
Steam reforming of methane ( CHA) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 75.0 L tank with 34. mol of methane gas and 14. mol of water vapor, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 4.2 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K.- Explanation Check 2021 McGraw H E MacBook Air F10 F7 esc F3 F2 * # 2$ & @ 7 8
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