Given the reaction: 4 NH4 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) and an instantaneous rate of consumption for oxygen of -0.25 Ms-1, what will be the rate of formation of NO (g)?
Added by Gonzalo W.
Step 1
From the balanced equation, 5 moles of O2 are consumed to form 4 moles of NO. Show more…
Show all steps
Your feedback will help us improve your experience
Ronald Prasad and 61 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Consider the reaction 4NO2(g) + O2(g) → 2N2O5(g) At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0039 M/s. What rate is the molecular oxygen being consumed?
David C.
What is the rate of formation of I2 in the following reaction if the rate of formation of HI is 0.042 M/s? 2 HI (g) → H2 (g) + I2 (g) 2. Determine the rate of formation of H2O and the rate of disappearance of O2 if the rate of consumption of NH3 is 0.070 M/s. 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) Δ(H2O)/Δt = -Δ(O2)/Δt =
Sri K.
In the following reaction, the concentration of $\mathrm{N}_{2} \mathrm{O}_{4}$ in mol/L was measured at the end of the times shown. What is the initial rate of the reaction? $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g)$$
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD