we place 4.00 atm of SbCl5 in a 5.00-liter container at 400C and we allow the...
we place 4.00 atm of SbCl5 in a 5.00-liter container at 400C and we allow the reaction to attain equilibrium. The final total pressure is 5.8 atm.
SbCl5 (g) <--> SbCl3 (g) + Cl2 (g)
What is the equilibrium partial pressure of SbCl5 and what is the K value? How many grams of SbCl5 are present at equilibrium?
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we place 4.00 atm of SbCl5 in a 5.00-liter container at 400C and
we allow the...
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At 248 ºC and a total pressure of 1.00 atm the degree of dissociation of SbCl5(g)...
At 248 ºC and a total pressure of 1.00 atm the degree of dissociation of SbCl5(g) is alpha = 0.718 for the reaction SbCl5(g) ↔ SbCl3(g) + Cl2(g) . The degree of dissociation alpha is defined as: alpha = (number of moles of SbCl5 dissociated at equilibrium) / (original number of moles of SbCl5) . (a) What is the value of the equilibrium constant K(T) at 248 ºC and 1.00 atm? (b) What is the value of Kx (the equilibrium...
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Show all work for both questions.
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***Please type answer if possible*** GAS VOLUME STOICHIOMETRY PROBLEMS 1. The combustion of ethanol (C2H5OH) takes...
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Antimony pentachloride can dissociate into antimony trichloride and chlorine: SbCl5(g SbCl3(2)+Cl2) At 248 °C, the equilibrium constant in terms of pressures, Kp, for this dissociation reaction is 1.07. (o) If 15.00 g of antimony pentachloride is placed in a 14.99-L vessel and heated to 248 "C, what is the partial pressure of antimony trichloride when equilibrium is attained? atm (b) What fraction of antimony pentachloride is dissociated at equilibrium?
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Show all work for both questions.
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