NiO is to be reduced to nickel metal in an industrial process by use of the reaction NiO(s) + CO(g) = Ni(s) + CO₂(g) At 1600 K the equilibrium constant for the reaction is K₂ = 6.0 × 10². ▼ Part A A 46.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.10 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂ (g) in the reactor? Express your answer in atmospheres to two significant figures. P(CO₂) = Submit Part B m = 197| ΑΣΦ Submit Request Answer What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. IVE ΑΣΦΑ 1 3 Request Answer a C C ? ? g atm

NiO is to be reduced to nickel metal in an industrial process by use of the reaction NiO(s) + CO(g) = Ni(s) + CO₂(g) At 1600 K the equilibrium constant for the reaction is K₂ = 6.0 × 10². ▼ Part A A 46.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.10 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂ (g) in the reactor? Express your answer in atmospheres to two significant figures. P(CO₂) = Submit Part B m = 197| ΑΣΦ Submit Request Answer What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. IVE ΑΣΦΑ 1 3 Request Answer a C C ? ? g atm

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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