Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can reactwith itself to form another form of NOx, dinitrogen tetroxide.A chemical engineer studying this reaction fills a 75 L tank with 31. mol of nitrogen dioxide gas. When the mixture has come to equilibrium hedetermines that it contains 12. mol of nitrogen dioxide gas.The engineer then adds another 10. mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles ofdinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.molx10ХG

Step 1: GivenVolume of tank = 75 LInitial moles of NO2 = 31 molEquilibrium moles of NO2 = 12…

Answered: Nitrogen dioxide is one of the many…

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...

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Suppose a 500. mL flask is filled with 1.6 mol of N₂ and 0.40 mol of NO. The following reaction becomes possible: N₂(g) + O₂(g) 2NO(g) The equilibrium constant K for this reaction is 6.10 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. M X Ś
Nitrosyl bromide decomposes according to the equation given below. If 0.640 mole of NOBr is placed in a 1.00 L flask containing no NO or Br2 it is found that at equilibrium there is 0.460 mole of NOBr. What is the value of Kc for this reaction? 2 NOBr (g) → 2 NO (g) + Br2 (g) 1.38 x 10−2 7.26 7.12 x 10−3 3.52 x 10−2 28.4
Hydrogen and iodine react to form hydrogen iodide, like this: H₂(g) + I₂(g) → 2 HI(g) Use this chemical equation to answer the questions in the table below. Suppose 220. mmol of H₂ and 220. mmol of I₂ are added to an empty flask. How much HI will be in the flask at equilibrium? Suppose 175. mmol of HI are added to an empty flask. How much HI will be in the flask at equilibrium? None. Some, but less than 440. mmol. 440. mmol. More than 440. mmol. None. Some, but less than 175. mmol. O 175. mmol. More than 175. mmol. 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 14, mol of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that It contains 4.2 mol of nitrogen diaxide gas. The engineer then adds another 4.7 mel of nitrogen diaxide, 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.
Consider the following equilibrium: N₂O4(g) = 2NO2(g) A 1.00 L container is initially filled with 0.200 mol N₂O4At equilibrium, 0.160 mol NO₂are present. What is the equilibrium concentration of N₂O4? 0.120 mol/L 0. 040 mol/L O.0.160 mol/L 0.080 mol/L 0.100 mol/L
"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 125 L tank with 20. mol of carbon monoxide gas and 24. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.0 mol of carbon monoxide gas, 11. mol of water vapor and 13. mol of carbon dioxide. The engineer then adds another 7.0 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. mol
"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 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 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
Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(9)+H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 10.6 g H₂O 138.4 g HNO3 21.8 g NO 19.6 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = [] x10 ×
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Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Ch(g) =S,Cl½(g) + CC1,(g) When 1.14 mol of CS, and 4.80 mol of Clh are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.650 mol of CC14. How many moles of Cl are present at on equilibrium? Select one: O a. 0.490 mol O b. 2.85 mol O c. 3.50 mol O d. 0.650 mol O e. 1.43 mol e to search F3 F4 F5 F6 FZ FB F9 F10 F11 F12 Prise %24 E R T G H K B N M 立

A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?
After equilibrium is reached in the reaction of 6.30 g H2 with 150. g I2, analysis shows that the 1.00 L flask contains 64.0 g of HI. How many moles of H2, I2, and HI are present in this equilibrium mixture? What is the Keq for this reaction?

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