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 47. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 22. mol of nitrogen dioxide gas. The engineer then adds another 16. 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

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