Which of the following statements are correct? Above the critical pressure, only the solid phase of a pure substance can exist. Above the critical temperature, a gas may not be condensed to a liquid. At the critical point, three phases (gas, liquid, and solid) may coexist at equilibrium       II and III     I and II     II only     I and III

Try Again Your answer is incorrect. One or more numbers is not written as a subscript. Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4 NO(g) + 6H₂O(g) →4 NH3(g)+ 5 O₂(g) Write the pressure equilibrium constant expression for this reaction. 4 (PNH) (PO₂) (PNO") ("MO") Р 4 ΝΟ 3

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 500. mL flask with 4.0 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 1.6 atm of nitrogen dioxide gas. The engineer then adds another 2.0 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 5

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 5.0 L flask with 1.3 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 0.59 atm of nitrogen dioxide gas. The engineer then adds another 0.65 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. Answer Submitted: atm A 13

41.9 g of CO(g) and 19.7 g of H2O(g) are placed in a 12.5 L container at 700.0 K. The following reaction occurs: CO(g) + H2O (g) -> H2 (g) + CO2 (g) If Kc = 8.3, what is the concentration of each gas that is present at equilibrium?

If 35.0 grams of magnesium oxide reacts with 21.0 grams of iodic acid to form magnesium iodate and water at 55.0°C and 206.0 kpa. Determnine the volume of magnesium iodate. (hint this is a limiting and excess reactant problem) R= 0.08206 Lx atm/mol x K R- 8.314 Lx kpa/mol x K R= 62.4 Lx mmHg/mol x K O 0.790 L O 0.868 L O.0.0597 L O 1.25 L

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 5.0 L flask with 2.4 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 1.5 atm of nitrogen dioxide gas. The engineer then adds another 0.80 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.

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 5.0 L flask with 0.66 atm of ethylene gas and 0.58 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.42 atm of ethylene gas and 0.34 atm of water vapor. The engineer then adds another 0.22 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm

21. At 1000 K, initially pure NO2(g) decomposes according to 2 NO2(g) 2 NO(g) + O2(g) with an equilibrium constant, K = 158, when pressures are expressed in bar. At equilibrium, the partial pressure of O2 = 0.75 bar. What are the partial pressures (in bar) of NO(g) and NO2(g), respectively, at equilibrium at 1000 K? = A) 0.250, 1.0 × 10-¹ B) 0.75, 4.0 × 104 C) 0.125, 1.0 × 10-¹ D) E) 1.50, 1.0 × 10-¹ 1.50, 4.0 × 104

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 2.0 L flask with 4.5 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 1.3 atm of nitrogen dioxide gas. The engineer then adds another 1.5 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. 0 atm x10 X Ś