2. Consider the reaction A2 + B2 ⇌ 2AB. If the initial concentration of both A2...
2. Consider the reaction A2 + B2 ⇌ 2AB. If the initial concentration of both A2 and B2 is 4.0 M, and after 10 minutes the reaction appears to stop. The concentration of [A2] is now 2.0M.
a. Draw a graph of [A2] vs. time, over the span of 20 minutes.
b. On the same axes draw a graph of [B2] v time, over a span of 20 minutes.
c. On the same axes draw a graph of [AB] v time over a span of 20 minutes.
d. We can discuss the rate in terms of [A2], [B2], or [AB]. How are they related to each other?
- Δ[A2]/Δt = ?
e. What is the difference between Δ[A2]/Δt and d[A2]/dt ?
f. At t = 15 minutes has the reaction actually stopped? Explain your answer at the macroscopic level and the molecular level.
Homework Answers
![D The Given equilibrium is- (Reactant) Product A - Reactant TA equilibrium concentration (t=1s). concentration (m) 0 [B2] - A](http://img.homeworklib.com/questions/6a2c8830-d7a1-11eb-ab5c-3bf52b12a366.png?x-oss-process=image/resize,w_560)
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2. Consider the reaction A2
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Problem Statement: How can concentration changes affect a chemical reaction? I, Data Collection: EXPERIMENT # 1 : R BG RG B + + Initial Concentration-I 0.6 0.7 0.8 0.9 - 0.13 Concentration Change-C -0.17 - 0,17 0.17 Ending Concentration-E 0.43 0.53 0.97 1.07 Calculate the change in concentration of each of the substances in the reaction. In the space below, draw a plot of the concentration v. time and label the axes. Identify the chemical substance that corresponds to...
just one example/demonstration!
Data needed to be calculated is in highlighted in green boxes.
And I highlighted in red an equation (not sure if thats what you
use to calculate it) And ignore the lab instructions on completeing
a graph!! I already know how to do that in excel, just curious how
Ln (relative rate) and 1/T in K^-1 is calculated by hand*
here is the rest of that lab leading up to the question as I
know its typically...
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