Suppose a 250. mL flask is filled with 0.80 mol of O, and 0.40 mol of NO. This reaction becomes possible: N, (g) +0, (g) - 2NO(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. N2 02 NO initial change equilibrium

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

Consider the following reaction: 2NH3 (9) N2(g) + 3H₂ (9) = If 0.00148 moles of NH3(g), 0.268 moles of N₂, and 0.643 moles of H₂ are at equilibrium in a 11.7 L container at 932 K, the value of the equilibrium constant, Ke, is

Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.80 mol of NO and 0.70 mol of CO,. The following reaction becomes possible: 2' NO, (g) +CO(g) - NO(g)+CO,(g) The equilibrium constant K for this reaction is 6.92 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. olo Ar OM ?

Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 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 O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium

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 100 L tank with 45. mol of ethylene gas and 35. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 34. mol of ethylene gas and 24. mol of water vapor. The engineer then adds another 18. 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

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 50 L tank with 15. mol of ethylene gas and 22. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.8 mol of ethylene gas and 14.8 mol of water vapor. The engineer then adds another 5.5 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

Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(2)- -2NO(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 N,. You can leave out the M symbol for molarity. N2 O2 NO initial change equilibrium olo

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?

Suppose a 250. mL flask is filled with 1.4 mol of CO, 1.9 mol of H₂O and 1.0 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) 2 The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś ?