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Ch.15 - Chemical Equilibrium

Chapter 15, Problem 25c

At 1000 K, 𝐾𝑝 = 1.85 for the reaction SO2(𝑔) + 12 O2(𝑔) β‡Œ SO3(𝑔) (c) What is the value of 𝐾𝑐 for the reaction in part (b)?

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Hi everyone. So we have the action below. And the K. P. Value is 2.47. I'm sent to the third power or asked how the K. C. For the reaction at this temperature. Since we're asked to find the K. C. And we're giving the K. P. We're gonna need to use the occasion K. P. It was K. C. Times are T to the power of data. N. Where are as R gas constant T. Is our temperature in delta, N. Is the sum of the molds of the gaseous product minus is some of the molds of the gas is reacting. And if he rearranged this to solve for K. C, we get K. C equals K. P. About about R. T. The power of data. And so for K. P We're giving 2.47 lb 10 to the third. Okay. See is what we're looking for. Art is 0.08 leaders from atmosphere about about malls times kelvin. And for the temperature We have 1200 K. And for delta N. We have one mole of carbon monoxide. The three most passion gas -1 Mall of Methane Plus one more of H 20. Gas. Get two miles total. Now we can plug an advice into the equation. We get K. C. Equals 2.47 Times 10 to the 3rd, Divided by 0.08206. Later times atmosphere about about Moles Times Kelvin. I'm 1200 K. Into the power of two. Okay, see Is 0.255. Since K. C. Does not have any units, we can disregard the units. Thanks for watching my video, and I hope it was helpful.
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Which of the following statements are true and which are false? (c) As the value of the equilibrium constant increases, the speed at which a reaction reaches equilibrium must increase.

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If 𝐾𝑐 = 0.042 for PCl3(𝑔) + Cl2(𝑔) β‡Œ PCl5(𝑔) at 500 K, what is the value of 𝐾𝑝 for this reaction at this temperature?

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Textbook Question

Consider the following equilibrium: 2 H2(𝑔) + S2(β€Šπ‘”) β‡Œ 2 H2S(𝑔) 𝐾𝑐 = 1.08Γ—107 at 700Β°C (c) Calculate the value of 𝐾𝑐 if you rewrote the equation H2(𝑔) + 1/2 S2(β€Šπ‘”) β‡Œ H2S(𝑔)

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Textbook Question

Consider the following equilibrium, for which at 𝐾𝑝 = 0.0752 at 480Β°C: 2 Cl2(𝑔) + 2 H2O(𝑔) β‡Œ 4 HCl(𝑔) + O2(𝑔) (a) What is the value of 𝐾𝑝 for the reaction 4 HCl(𝑔) + O2(𝑔) β‡Œ 2 Cl2(𝑔) + 2 H2O(𝑔)?

Textbook Question

The following equilibria were attained at 823 K:

CoO(s) + H2(g) β†’ Co(s) + H2O(g) Kc = 67

CoO(s) + CO(g) β†’ Co(s) + CO2(g) Kc = 490

Based on these equilibria, calculate the value of 𝐾𝑐 for H2(𝑔)β€Šβ€Š+ CO2(𝑔) β‡Œ CO(𝑔) + H2O(𝑔) at 823 K.

Textbook Question

Consider the equilibrium N2(𝑔) + O2(𝑔) + Br2(𝑔) β‡Œ 2 NOBr(𝑔) Calculate the equilibrium constant 𝐾𝑝 for this reaction, given the following information at 298 K:

2 NO(𝑔) + Br2(𝑔) β‡Œ 2 NOBr(𝑔) 𝐾𝑐 = 2.02

NO(𝑔) β‡Œ N2(𝑔) + O2(𝑔) 𝐾𝑐 = 2.1Γ—1030

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