A 10-liter container is filled with 0.10 mol of H2( g) and heated to 3000 K, causing some of t

step 1 In this question we would like to determine the partial pressure of hydrogen. And we know the pa

A 10-liter container is filled with 0.10 mol of H2( g) and...

A 10-liter container is filled with $0.10 \mathrm{~mol}$ of $\mathrm{H}_{2}(\mathrm{~g})$ and heated to $3000 \mathrm{~K}$, causing some of the $\mathrm{H}_{2}(g)$ to decompose into $\mathrm{H}(g)$. The pressure is found to be $3.0 \mathrm{~atm}$. Find the partial pressure of the $\mathrm{H}(\mathrm{g})$ that forms from $\mathrm{H}_{2}$ at this temperature. (Assume two significant figures for the temperature.)

Key Concepts

Reaction Stoichiometry and Chemical Equilibrium

Reaction stoichiometry describes the quantitative relationships between reactants and products in a chemical reaction. In gas phase reactions, particularly those involving decomposition or dissociation (such as a diatomic molecule breaking into atoms), the stoichiometry affects the total number of gas particles and thus the pressure. When a system reaches chemical equilibrium after such a reaction, the relative amounts of reactants and products determine the individual partial pressures and need to be analyzed using stoichiometric relationships.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) relates pressure, volume, temperature, and amount of gas. It is fundamental in predicting how a gas behaves under various conditions and is used to calculate the total number of moles in a system when temperature, pressure, and volume are known. This concept is essential for understanding the overall behavior of gases in a closed container regardless of any chemical reactions occurring within the system.

Partial Pressure

Partial pressure is the pressure that each individual gas in a mixture would exert if it alone occupied the entire volume at the same temperature. Dalton's Law of Partial Pressures states that the total pressure of a gas mixture is the sum of the partial pressures of all the components. This concept is crucial in analyzing gas-phase reactions and determining the contribution of each species to the total pressure in equilibrium systems.

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