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18 Nov 2019
Why wouldn't part 4 be .216??
11.1 g of NH_4 HS(s) were added to a 0.800 L evacuated flask. In the flask, the solid under goes the reaction: NH_4 HS(s) doubleheadarrow NH_3(g) + H_2 S(g) At 30 degree C the value of the equilibrium constant is K_P = 0.388. When the system reaches, equilibrium determine the following quantities: Partial pressure of NH_3 (g) is .622 atm. Total pressure in the container is 1.244 atm the concentration of NH_3 (g) is .012 M The amount of NH_4 SH(s) that has decomposed is moles
Why wouldn't part 4 be .216??
11.1 g of NH_4 HS(s) were added to a 0.800 L evacuated flask. In the flask, the solid under goes the reaction: NH_4 HS(s) doubleheadarrow NH_3(g) + H_2 S(g) At 30 degree C the value of the equilibrium constant is K_P = 0.388. When the system reaches, equilibrium determine the following quantities: Partial pressure of NH_3 (g) is .622 atm. Total pressure in the container is 1.244 atm the concentration of NH_3 (g) is .012 M The amount of NH_4 SH(s) that has decomposed is moles
Keith LeannonLv2
2 Jun 2019