A mixture of 0.498 M H2O , 0.358 M Cl2O , and 0.742 M HClO are enclosed in a vessel at 25°C .   H2O(g)+Cl2O(g)↽−−⇀2HOCl(g)?c=0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25°C

Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375 X (b) What is Kp if the total pressure is 10.5 atm? 9.12

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas. PCl3(g) + Cl2(g)  PCl5(g). A gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.128 atm, PCl2 = 0.141 atm, and PPCl5 = 1.21 atm. (a) What is the value of Kp at this temperature? ______ (b) Does the equilibrium favor reactants or products? The equilibrium favors products. The equilibrium favors reactants.     Neither reactants nor products are favored.

Hh.53.

Determine the equilibrium partial pressure of NH3 in a reaction vessel that initially contained 0.900 atm N2 and 0.500 atm H2 at 648 K.

Methanol is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen: CO(g) + 2 H­2(g) <-> CH3OH(g). At equilibrium mixture in a 1.05 L vessel is found to contain 0.652 mol CH3OH, 0.386 mol CO, and 0.209 mol H2.  Calculate the value of Kc.

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