## Reaction Rates and Stoichiometry

In this latest blog post, “Unveiling the Dynamics: Understanding Reaction Rates and Stoichiometry in NH₃ Decomposition,” we delve into the intricacies of a chemical reaction involving ammonia (NH₃). Breaking down the balanced equation

** 2NH₃(g) → N₂(g) + 3H₂(g)**,

We explore how stoichiometry plays a pivotal role in determining the rate of change of reactants and products. With a focus on the rate of change of ammonia ** (A[NH₃]/Δt)**, we decipher the significance of stoichiometric coefficients and their impact on reaction kinetics.

## Question

Can you explain what the rate ** A[NH₃]/Δt** is, given the reaction

**and a known rate**

*2NH₃(g) → N₂(g) + 3H₂(g)*

*A[H₂]/Δt of 0.030 mol/s?*## Answer:

To determine the rate of A[NH₃]/Δt (rate of change of concentration of NH₃ over time), you can use the stoichiometry of the reaction. Given the reaction:

*2NH3(g)→N2(g)+3H2(g)*

If the rate of change of ** [H₂] (A[H₂]/Δt)** is given as

**, you can use the stoichiometric coefficients to find the rate of change of**

*0.030 mol/s***.**

*[NH₃] (A[NH₃]/Δt)**A[NH₃]/A[H₂]=Coefficient of NH₃/Coefficient of H₂*

*A[NH₃]/A[H₂]=1/3*

Now, multiply the given rate ** A[H₂]/Δt** by this ratio to find

**:**

*A[NH₃]/Δt**A[NH₃]/A[H₂]×A[H₂]/Δt=1/3×0.030 mol/s*

*A[NH₃]/Δt=0.010 mol/s*

###
*Final Answer: *

Therefore, the rate of change of *[NH3] (A[NH₃]/Δt) is 0.010 mol/s0.010mol/s.*

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