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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 2NH₃(g) → N₂(g) + 3H₂(g) and a known rate 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)
The coefficients in the balanced chemical equation give the molar ratios of reactants and products. In this case, the ratio of NH₃ to H₂ is 2:3.
If the rate of change of [H₂] (A[H₂]/Δt) is given as 0.030 mol/s, you can use the stoichiometric coefficients to find the rate of change of [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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