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Ch.15 - Chemical Equilibrium
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 57
Chapter 15, Problem 57

For the reaction I2(g) + Br2(g) ⇌ 2 IBr(g), Kc = 280 at 150 _x001F_C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150 _x001F_C. What are the equilibrium concentrations of IBr, I2, and Br2?

Verified step by step guidance
1
Step 1: Write the balanced chemical equation for the reaction: I2(g) + Br2(g) ⇌ 2 IBr(g).
Step 2: Define the initial concentrations of the reactants and products. Since 0.500 mol of IBr is placed in a 2.00 L flask, the initial concentration of IBr is 0.500 mol / 2.00 L = 0.250 M. The initial concentrations of I2 and Br2 are both 0 M.
Step 3: Set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentrations. Let x be the change in concentration of I2 and Br2 that reacts to form IBr. The changes in concentration will be: I2: +x, Br2: +x, IBr: -2x.
Step 4: Express the equilibrium concentrations in terms of x: [I2] = x, [Br2] = x, [IBr] = 0.250 - 2x.
Step 5: Use the equilibrium constant expression Kc = [IBr]^2 / ([I2][Br2]) = 280 to solve for x. Substitute the equilibrium concentrations into the expression and solve for x to find the equilibrium concentrations of I2, Br2, and IBr.
Related Practice
Open Question
Consider the reaction \( \text{CaSO}_4(\text{s}) \rightleftharpoons \text{Ca}^{2+}(\text{aq}) + \text{SO}_4^{2-}(\text{aq}) \) At 25 °C, the equilibrium constant is \( K_c = 2.4 \times 10^{-5} \) for this reaction. (a) If excess \( \text{CaSO}_4(\text{s}) \) is mixed with water at 25 °C to produce a saturated solution of \( \text{CaSO}_4 \), what are the equilibrium concentrations of \( \text{Ca}^{2+} \) and \( \text{SO}_4^{2-} \)? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of \( \text{CaSO}_4(\text{s}) \) needed to achieve equilibrium?
Textbook Question

At 80°C, 𝐾𝑐 = 1.87×10−3 for the reaction PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80°C and decomposes until equilibrium is reached.

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Textbook Question

At 80°C, 𝐾𝑐 = 1.87×10−3 for the reaction PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80°C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the minimum mass of PH3BCl3(𝑠) that must be added to the flask to achieve equilibrium?

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Textbook Question

At 25°C, the reaction CaCrO4(𝑠) ⇌ Ca2+(𝑎𝑞) + CrO42−(𝑎𝑞) has an equilibrium constant 𝐾𝑐 = 7.1×10−4. What are the equilibrium concentrations of Ca2+ and CrO42− in a saturated solution of CaCrO4?

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Open Question
Methane, CH4, reacts with I2 according to the reaction CH4(g) + I2(g) ⇌ CH3I(g) + HI(g). At 630 K, Kp for this reaction is 2.26 × 10^-4. A reaction was set up at 630 K with initial partial pressures of methane at 105.1 torr and I2 at 7.96 torr. Calculate the pressures, in torr, of all reactants and products at equilibrium.
Textbook Question

Consider the following equilibrium, for which Δ𝐻<0

2 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)

(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO3(𝑔) is removed from the system?

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