CHM 2046 Chapter Notes - Chapter 16: Rate Equation, Reaction Rate, Joule

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Published on 19 Jul 2019
School
University of Florida
Department
Chemistry
Course
CHM 2046
Question 1
1 / 1 pts
Balance the following equation and express the rate in terms of the change in
concentration with time for each substance: NO(g) + O2(g) N2O3 (g)
When N2O3 is forming at 0.112 M/s, at what rate is NO decreasing? Enter a positive
number to 3 decimal places.
(MTS 5/4/2018)
0.224
When the equation is balanced, the reactant to product ratio is 1:2, so if the product
forms at 0.112, the reactant is consumed at twice that rate.
Question 2
1 / 1 pts
Give the individual reaction orders for all substances and the overall reaction order
from the following rate law: rate=k[BrO3−][Br−][H+]2
1 order in bromate ions
1 order in bromide ions
2 order in hydrogen ions
4 overall order of the reaction
(MTS 5/4/2018)
Answer 1:
1
Answer 2:
1
Answer 3:
2
Answer 4:
4
Question 3
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1 / 1 pts
For the reaction H2SeO3(aq) + 6 I (aq) + 4 H +(aq) Se(s) + 2I3
(aq) + 3 H2O(l) at 0°C, the following data were obtained:
Exp
initial rate (M/s)
initial H2SeO3 (M)
initial I (M)
iniital H+ (M)
1
9.85e-7
0.0025
0.015
0.015
2
7.88e-6
0.0025
0.030
0.015
3
3.94e-6
0.010
0.015
0.015
4
3.15e-5
0.0025
0.030
0.030
order in H2SeO3 (enter a whole number)
order in iodide ion (enter a whole number)
order in hydrogen ion (enter a whole number)
overall order of the reaction (enter a whole number)
what is value of k? Enter a number to 2 sig figs e.g. 1.2e3
Answer 1:
1
Answer 2:
3
Answer 3:
2
Answer 4:
6
Answer 5:
5.2e5
For 1-3 use the row where all are constant except what you test (Mpers/Mpers =
M/M) and for 5, plug in a full row (initial rate M/s = k (H2SeO3)^x(I)^x(H)^x)
IncorrectQuestion 4
0 / 1 pts
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The scenes below show two experiments at a given temperature and volume involving
reactants X (black) and Y (green):
If the rate law for the reaction is rate = k[X]22 what is the initial rate of experiment 2
given that the rate of experiment 1 is 0.50 M/s
(MTS 5/4/2018)
0.50 M/s
0.056 M/s
0.25 M/s
1.0 M/s
0.75 M/s
0.10 M/s
**Answer is NOT 0.25!
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Document Summary

Balance the following equation and express the rate in terms of the change in concentration with time for each substance: no(g) + o2(g) n2o3 (g) Enter a positive number to 3 decimal places. (mts 5/4/2018) When the equation is balanced, the reactant to product ratio is 1:2, so if the product forms at 0. 112, the reactant is consumed at twice that rate. Give the individual reaction orders for all substances and the overall reaction order from the following rate law: rate=k[bro3 ][br ][h+]2. 4 overall order of the reaction (mts 5/4/2018) (aq) + 3 h2o(l) at 0 c, the following data were obtained: Enter a number to 2 sig figs e. g. 1. 2e3. For 1-3 use the row where all are constant except what you test (mpers/mpers = M/m) and for 5, plug in a full row (initial rate m/s = k (h2seo3)^x(i)^x(h)^x)