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The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.
2 SO2(g) + O2(g) ? 2 SO3(g) Kc = 1.7 × 106SO3(g) ? 1/2 O2(g) + SO2(g) Kc = ?
The equilibrium constant is equal to 5.00 at 1300 K for the reaction:
2 SO2(g) + O2(g) ? 2 SO3(g).
If initial concentrations are [SO2] = 1.20 M, [O2] = 0.45 M, and [SO3] = 1.80 M, the system is not at equilibrium and will shift to the right to achieve an equilibrium state. not at equilibrium and will shift to the left to achieve an equilibrium state. at equilibrium. not at equilibrium and will remain in an unequilibrated state.
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Sample were collected in a zinc smelter to determine the exposure of a furnace tender to lead fume during his normal work duties which involves "furnace draws" and general activities around the furnace.
Calculate ΔG for the reaction if the partial pressures of the initial mixture are PPCl5 = 0.0029 atm, PPCl3 = 0.27 atm, and PCl2 = 0.40 atm PCl5(g)--> PCl3(g) + Cl2(g)
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Tarnish (silver sulfide) may be removed from a silver spoon by placing the spoon in contact with a metallic container holding a solution of baking soda.
A gaseous mixture of O2 and Kr has a density of 1.184 g/L at 385 torr and 300. K. What is the mole percent O2 in the mixture?
potassiumm chlorate (KClO3) decomposes to form potassium chloride and oxygen gas. if 5.4 moles of potassium chlorate decompose, how many moles of oxygen could be produce.
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A 1L flask is filled with 1.00 g of argon at 25 C . A sample of ethane vapor is added to the same flask until the total pressure is 1.20 atm. What is partial pressure of Argon and ethane in the flask?
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