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"A 1-L flask is filled with 1.45 g of argon at 25 ∘C. A sample of ethane vapour is added to the same flask until the total pressure is 1.11 bar ."
(A) What is the partial pressure of Argon PAr , in the flask?
(B) What is the partial pressure of ethane, Pethane , in the flask?
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- Consider the reaction: 2 NO(g) + Br2(g) =2 NOBI(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br2) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBR at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L·bar/mol·K and MW of Br2 is 159.808 g/mol.) Calculate the Kp.A gas mixture used for anesthesia contains 2.83 mol oxygen, O2, and 8.41 mol nitrous oxide, N2O. The total pressure of the mixture is 192 kPa.(a) What are the mole fractions of O2 and N2O?(b) What are the partial pressures of O2 and N2O?Consider the reaction: 2 NO(g) + Br2(g) =2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br2) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBR at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L·bar/mol· K and MW of Br2 is 159.808 g/mol.) Calculate the Kp. Incorrect, 1 attempt remaining Your submission: Feedback: Use PV=nRT to determine the initial pressures of the reactants. You can then determine the pressures of the reactants equilibrium by subtracting the pressure that reacted. Kp = P(NOBr)*/P(NO)²*P(Br)2 43.8 %3D
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