NiO is to be reduced to nickel metal in an industrial process by use of thereactionNiO (s) + CO(g)Ni(s) + CO₂(g)-At 1800 K the equilibrium constant for the reaction is Kp = 6.0 x 10²▼Part AA 52.0-L reactor at 1600 K is charged with 50.0 g of NiO (s) and 1.50 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.ΠΙΑΣΦP(CO₂) =SubmitPart BRequest AnswerSubmitWhat mass of Ni(s) is produced in the reaction in part (a)?Express your answer in grams to two significant figures.ΠΑΣΦ+Request AnswerA??Review | Constants | Periodic Tableatm

#Part-A: The equilibrium reaction is: NiO(s) + CO(g) ⇌ Ni(s) + CO2(g) ; Kp = 6.0*102

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 x 10² Part A A 52.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.50 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂ (R) in the reactor? Express your answer in atmospheres to two significant figures. VE ΑΣΦ P(CO₂) = Submit Part B M == Request Answer What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. VE ΑΣΦ Submit A C Request Answer ? ? R 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 x 10² Part A A 52.0-L reactor at 1600 K is charged with 50.0 g of NiO(s) and 1.50 atm of CO(g). After equilibrium is reached, what is the partial pressure of CO₂ (R) in the reactor? Express your answer in atmospheres to two significant figures. VE ΑΣΦ P(CO₂) = Submit Part B M == Request Answer What mass of Ni(s) is produced in the reaction in part (a)? Express your answer in grams to two significant figures. VE ΑΣΦ Submit A C Request Answer ? ? R atm

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 54QAP: Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When...

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