Consider the following reaction: 2CH,Cl2(g) CH4(g) + CC14(g) If 0.725 moles of CH,Cl,(g), 0.610 moles of CH4, and 0.658 moles of CCl, are at equilibrium in a 15.1 L container at 589 K, the value of the equilibrium constant, Ke, is

A mixture of 30.0 mol of NO(g) and 18.0 mol of O2(g) is placed in an empty 3.00-liter flask held at a constant temperature. These gases react until the reaction represented below comes to equilibrium. At equilibrium, the vessel contains 26.4 moles of NO2. What is the value of the equilibrium constant at the constant temperature? 2NO(g) + O2(g)  2NO2(g)

While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 mol of ethylene, 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 X

Consider the following reaction:2HI(g) H2(g) + I2(g)If 2.04 moles of HI(g), 0.232 moles of H2, and 0.369 moles of I2 are at equilibrium in a 19.4 L container at 752 K, the value of the equilibrium constant, Kc, is .