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Ch.15 - Chemical Equilibrium
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 87
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Chapter 15, Problem 87

NiO is to be reduced to nickel metal in an industrial process using the reaction NiO(s) + CO(g) ⇌ Ni(s) + CO2(g). At 1600 K, the equilibrium constant for the reaction is Kp = 6.0 × 10^2. If a CO pressure of 150 torr is to be employed in the furnace and the total pressure never exceeds 760 torr, will reduction occur?

Verified step by step guidance
1
Step 1: Write the expression for the equilibrium constant Kp for the reaction. For the reaction NiO(s) + CO(g) ⇌ Ni(s) + CO2(g), the expression is Kp = (P_CO2) / (P_CO), where P_CO2 and P_CO are the partial pressures of CO2 and CO, respectively.
Step 2: Identify the given values. You are given Kp = 6.0 × 10^2 and the pressure of CO, P_CO = 150 torr. The total pressure is not to exceed 760 torr.
Step 3: Calculate the partial pressure of CO2, P_CO2, using the equilibrium constant expression. Rearrange the expression to find P_CO2 = Kp × P_CO.
Step 4: Check if the calculated P_CO2, when added to the given P_CO, exceeds the total pressure limit of 760 torr. If P_CO2 + P_CO ≤ 760 torr, the reduction will occur under the given conditions.
Step 5: Conclude whether the reduction of NiO to Ni will occur based on the comparison of the calculated total pressure with the maximum allowable pressure.
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Textbook Question

At 900 °C, 𝐾𝑐 = 0.0108 for the reaction

CaCO3(𝑠) ⇌ CaO(𝑠) + CO2(𝑔)

A mixture of CaCO3, CaO, and CO2 is placed in a 10.0-L vessel at 900°C. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium?

(c) 30.5 g CaCO3, 25.5 g CaO, and 6.48 g CO2

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Open Question
When 1.50 mol CO2 and 1.50 mol H2 are placed in a 3.00-L container at 395 _x001F_C, the following reaction occurs: CO2(g) + H2(g) ⇌ CO(g) + H2O(g). If Kc = 0.802, what are the concentrations of each substance in the equilibrium mixture?
Textbook Question

The equilibrium constant constant 𝐾𝑐 for C(𝑠) + CO2(𝑔) ⇌ 2 CO(𝑔) is 1.9 at 1000 K and 0.133 at 298 K. (b) If excess C is allowed to react with 25.0 g of CO2 in a 3.00-L vessel at 1000 K, how many grams of C are consumed?

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Open Question
What does this anecdote tell us about the equilibrium constant for the reaction of iron oxide with carbon monoxide to produce elemental iron and CO2?
Textbook Question

At 700 K, the equilibrium constant for the reaction CCl4(𝑔) ⇌ C(𝑠) + 2 Cl2(𝑔) is 𝐾𝑝 = 0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K. (b) What are the partial pressures of CCl4 and Cl2 at equilibrium?

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Open Question
An equilibrium mixture of H2, I2, and HI at 458 _x001F_C contains 0.112 mol H2, 0.112 mol I2, and 0.775 mol HI in a 5.00-L vessel. What are the equilibrium partial pressures when equilibrium is reestablished following the addition of 0.200 mol of HI?