Explanation Given: T=175K;P NO =522 torr;p O2 =421 torr; P T =748 torr. Formula used: K p = [ PNO2 ] 2 [ PNO ] 2 [ PO2 ] Calculation: (a) We are given the initial partial pressures of NO and O 2 and we know the total pressure of the system at equilibrium. These values can be used to solve for K p . We can set up an ICE table and solve for the equilibrium pressures: NO O 2 NO 2 I 522 421 0 C -2 x -x +2 x E 522–2 x 421– x 2 x We can insert the equilibrium partial pressures into the total pressure formula to solve for x : p T + P NO + P O2 + P NO2 748=(522-2x)+(412-x)+2x 748=934-x x=186 torr Now, we can find the partial pressures of each substance at equilibrium and insert these values into the K p expression to solve for K p: P NO =522-2(186)=150 torr P O2 =421-186=235 torr P NO2 =2(186)=372 torr K p =

Chemistry: Structure and Properties Plus MasteringChemistry with eText -- Access Card Package

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Chapter 16, Problem 93E

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To determine: Find the Kp of the reaction and use that value to find the partial pressures at equilibrium.

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Chapter 16, Problem 92E

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Chemistry: Structure and Properties Plus MasteringChemistry with eText -- Access Card Package

Ch. 16 - What is the correct expression for the equilibrium...Ch. 16 - Prob. 2SAQ Ch. 16 - Use the data below to find the equilibrium...Ch. 16 - The reaction shown here has a Kp = 4.5X102 AT 825...Ch. 16 - Consider the reaction between NO and Cl2 to form...Ch. 16 - Prob. 6SAQ Ch. 16 - Consider the reaction between iodine gas and...Ch. 16 - Prob. 8SAQ Ch. 16 - The decomposition of NH4HS is endothermic:...Ch. 16 - The solid XY decomposes into gaseous X and Y:...

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Find the K p of the reaction and use that value to find the partial pressures at equilibrium.

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