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Ch.15 - Chemical Equilibrium
All textbooksMcMurry 8th EditionCh.15 - Chemical EquilibriumProblem 89
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Chapter 15, Problem 89

Gaseous indium dihydride is formed from the elements at elevated temperature: ln(g) + H2(g) ightarrow lnH2(g), Kp = 1.48 at 973 K. Partial pressures measured in a reaction vessel are: P_in = 0.0600 atm, P_H2 = 0.0350 atm, P_lnH2 = 0.0760 atm. (b) Determine the equilibrium partial pressures of all the gases.

Verified step by step guidance
1
Step 1: Write the expression for the equilibrium constant Kp for the reaction: \( \text{In}(g) + \text{H}_2(g) \rightleftharpoons \text{InH}_2(g) \). The expression is given by \( K_p = \frac{P_{\text{InH}_2}}{P_{\text{In}} \times P_{\text{H}_2}} \).
Step 2: Substitute the given partial pressures into the Kp expression: \( K_p = \frac{0.0760}{0.0600 \times 0.0350} \). Calculate this value to check if the system is at equilibrium.
Step 3: Compare the calculated Kp value with the given Kp (1.48). If they are equal, the system is at equilibrium. If not, determine the direction in which the reaction will shift to reach equilibrium.
Step 4: If the reaction is not at equilibrium, use an ICE (Initial, Change, Equilibrium) table to determine the changes in partial pressures needed to reach equilibrium. Define the change in pressure as \( x \) and adjust the initial pressures accordingly.
Step 5: Substitute the equilibrium expressions from the ICE table back into the Kp expression and solve for \( x \). Use this value to find the equilibrium partial pressures of all gases.
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