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.

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the partial pressures of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction ln(g) + H2(g) ⇌ lnH2(g), Kp = 1.48 indicates the relationship between the partial pressures of indium dihydride and its constituent gases. Understanding Kp is essential for calculating the equilibrium state of the system.

Partial pressure is the pressure exerted by a single component of a gas mixture. In this context, the partial pressures of indium (P_in), hydrogen (P_H2), and indium dihydride (P_lnH2) are crucial for determining the equilibrium state of the reaction. The total pressure of the gas mixture is the sum of the partial pressures, and these values are used to calculate the equilibrium concentrations.

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In this case, if the partial pressures of the reactants or products are altered, the system will shift in the direction that minimizes the effect of that change, which is vital for predicting how the equilibrium will shift in response to changes in partial pressures.