CO(g ) + H2O(g ) <---> CO2(g ) + H2(g ), Kc = 0.0611 at 2000 K . A reaction mixture initially contains a CO partial pressure of 2.50 atm, an H2O partial pressure of 2.50 atm, a CO2 partial pressure of 1.00 atm, and an H2 partial pressure of 1.00 atm at 2000 K. Calculate the equilibrium partial pressure of CO

In a sample of oxygen gas at room temperature, the average kinetic energy of all the balls stays constant. which postulate of kinetic molecular theory best explains how this is possible? a. attractive forces between gas particles are negligible because the particles of an ideal gas are moving so quickly. b. collisions between gas particles are elastic; there is no net gain or loss of kinetic energy. c. gases consist of a large number of small particles, with a lot of space between the particles. d. gas particles are in constant, random motion, and higher kinetic energy means faster movement.

Which statement correctly describes metallic bonds? a. they form when certain atoms lose electrons and other atoms gain electrons. b. they involve an attraction between anions and cations. they always involvpoth a metal and a nonmetal. d. they can only form between atoms of the same element. e. they form because electrons can move freely between atoms.

How many grams of magnesium metal will react completely with 8.3 liters of 5.5m hcl? show all work