The equilibrium constant value for the reaction N2( g)+3 H2( g) ⇌2 NH3( g) is 1.48 ×10^-5, the v

step 1 In this problem we have given that the equilibrium constant value for the reaction N2 reacts wit

The equilibrium constant value for the reaction N2( g)+3...

The equilibrium constant value for the reaction $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$ is $1.48 \times 10^{-5}$, the value for the reaction $1 / 2 \mathrm{~N}_2(\mathrm{~g})+3 / 2 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{NH}_3(\mathrm{~g})$ is $\mathrm{n} \times 10^{-3}$ where n is (a) 1.85 (b) 3.85 (c) 4.85 (d) 10

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Equilibrium Constant

The equilibrium constant is a numerical value that expresses the ratio of the concentrations or partial pressures of products to reactants when a chemical reaction is at equilibrium. It quantitatively describes the extent of the reaction and is dependent on temperature.

Reaction Stoichiometry Scaling

When a chemical reaction is modified by multiplying or dividing its stoichiometric coefficients by a constant factor, the equilibrium constant is affected by being raised to the power of that factor. This principle is crucial when comparing reactions written in different forms.

Mathematical Transformation of Equilibrium Constants

The process of adjusting the equilibrium constant when the reaction equation is scaled involves applying a power law transformation. Specifically, if the entire reaction is multiplied by a factor, the new equilibrium constant is the original constant raised to the power of that factor, allowing for straightforward recalculation between different representations of the same chemical reaction.

Transcript

Please give Ace some feedback