In the synthesis of ammonia, if -Δ[H2] / Δt=4.5 ×10^-4 mol / L ·min, what is Δ[NH3] / Δt ? N2(g)

Name: Problem 4, Chapter 15: Chemistry and Chemical Reactivity
Uploaded: 2020-06-08T00:39:18-08:00
Duration: 1 min 35 s
Channel: Will Li
Description: In the synthesis of ammonia, if -Δ[H2] / Δt=4.5 ×10^-4 mol / L ·min, what is Δ[NH3] / Δt ? N2(g)+3 H2(g) ⟶2 NH3(g)

step 1 This problem, we're trying to determine what is the rate of appearance of NH3, given that the ra

This problem has been solved

by verified expert Will Li

100% free to try

Question

In the synthesis of ammonia, if $-\Delta\left[\mathrm{H}_{2}\right] / \Delta t=4.5 \times 10^{-4}$ $\mathrm{mol} / \mathrm{L} \cdot \mathrm{min},$ what is $\Delta\left[\mathrm{NH}_{3}\right] / \Delta t ?$ $\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})$

   In the synthesis of ammonia, if $-\Delta\left[\mathrm{H}_{2}\right] / \Delta t=4.5 \times 10^{-4}$ $\mathrm{mol} / \mathrm{L} \cdot \mathrm{min},$ what is $\Delta\left[\mathrm{NH}_{3}\right] / \Delta t ?$ $\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})$

Chemistry and Chemical Reactivity

John C. Kotz, Paul… 6th Edition

Chapter 15, Problem 4

Instant Answer

Solved by Expert Will Li

06/08/2020

Step 1

5 \times 10^{-4}$ $\mathrm{mol} / \mathrm{L} \cdot \mathrm{min}$. Show more…

Show all steps

Thanks for your feedback!

In the synthesis of ammonia, if $-\Delta\left[\mathrm{H}_{2}\right] / \Delta t=4.5 \times 10^{-4}$ $\mathrm{mol} / \mathrm{L} \cdot \mathrm{min},$ what is $\Delta\left[\mathrm{NH}_{3}\right] / \Delta t ?$ $\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})$

Play audio

Feedback

Will Li and 72 other subject Chemistry 101 educators are ready to help you.

Ask a new question

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

Reaction Rate in Chemical Kinetics

The reaction rate quantifies how quickly the concentration of a substance changes over time. This concept is central to kinetics, where the rate of disappearance for a reactant or appearance for a product is calculated based on changes in concentration per unit time, often using the stoichiometric relationships from the balanced equation.

Stoichiometric Relationships

Balanced chemical equations provide the mole ratios between reactants and products. These ratios allow us to convert the rate of consumption of one reactant into the rate of formation of a product by using the coefficients from the chemical equation.

Please give Ace some feedback