A United Nations toxicologist studying the properties of mustard gas, S(CH2CH2CI)2, a blistering agent used in warfare, prepares a mixture of 0.675 M SCI2 and 0.973 M C2H4 and allows it to react at 20.0°C: SCI2(g) + 2 C2H4(g) = S(CH2CH2CI)2(g) At equilibrium, [S(CH2CH2CI)2] = 0.350 M. Calculate Kc. 0.0692 0.0249 2.77 14.4 1.73

A mixture of 0.450 M H2, 0.473 M I2, and 0.926 M HI is enclosed in a vessel and heated to 430 °C.   H2(g)+I2(g)↽−−⇀2HI(g)?c=54.3 at 430 ∘C Calculate the equilibrium concentrations of each gas at 430 ∘C .

While ethanol (CH3CH,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 500. mL flask with 0.77 atm of ethylene gas and 0.98 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.34 atm of ethylene gas and 0.55 atm of water vapor. The engineer then adds another 0.19 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

For this equilibrium system, 2SO3(g) 2 25O2(g) + O2(g), Kc = 0.00407. At equilibrium, you would expect to find %3D relatively more products than reactant. relatively more reactant than products. about comparable amounts of reactant and products. no way to decide.