The reaction 2 N;Os - 2 N20. + Oz has a rate constant k= 0.055 min". If the initial concentration of N2Os is 0.980 M, what will be the concentration of N;Os after 10 minutes?ss
The reaction 2 N;Os - 2 N20. + Oz has a rate constant k= 0.055 min". If the initial concentration of N2Os is 0.980 M, what will be the concentration of N;Os after 10 minutes?ss
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![HELPFUL INFORMATION
MOLARITY (M) = # OF MOLES OF SOLUTELITERS OF SOLUTION
MOLALITY (m) – # OF MOLES OF SOLUTE/KG OF SOLVENT
density of water = 1.00g/ml R= 8.314 J/mole K R=0.08201 L atm/mole K K= "C + 273
AT - Kb x m (boiling point elevation)
AT, =i K, x m (boiling point elevation for electrolytes)
AT= Kr x m (freezing point depression)
AT=iK, x m (freezing point depression for electrolytes)
II = MRT ( II = osmotic pressure) - nonelectrolytes (organic compounds)
electrolytes
Il =i MRT
ARRHENIUS EQUATION: In k --E/RT + In A
k- Ae KT (T- Absolute Temperature,
k = rate constant, E.= Activation Energy, A = Frequency factor, R= gas constant)
In(kl/k2) = E/R (1/T2-1/T1) Please use at least 3 significant digits in your calculations.
Summary of Rate Laws for Zero-, First-, and Second-Order Reactions
Zero-Order
First-Order
Second-Order
rate law
rate -k
rate - RJAJ
rate - AA
units of rate constant
Ms
s1
M's-1
integrated rate law
[A] = -kt + [A],
In[A] = -kt + In[A], = kt + ()
plot needed for inear ft of rate data
JAl ve. I
nA va.
vs. t
relationship between slope of linear plot and rate
k- -slope
k- -slope
k= slope
constant
half-ite
fa =
f =
The reaction 2 N2Os + 2 N204 + O2 has a rate constant k= 0.055 min. If the
initial concentration of N2Os is 0.980 M, what will be the concentration of N2Os
after 10 minutes?ss](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fef4897a5-2d0a-4dff-bcc1-4f1af9f3eb36%2Fa923b701-e859-44e1-9ca5-4a52f69906c6%2Flgubq4_processed.png&w=3840&q=75)
Transcribed Image Text:HELPFUL INFORMATION
MOLARITY (M) = # OF MOLES OF SOLUTELITERS OF SOLUTION
MOLALITY (m) – # OF MOLES OF SOLUTE/KG OF SOLVENT
density of water = 1.00g/ml R= 8.314 J/mole K R=0.08201 L atm/mole K K= "C + 273
AT - Kb x m (boiling point elevation)
AT, =i K, x m (boiling point elevation for electrolytes)
AT= Kr x m (freezing point depression)
AT=iK, x m (freezing point depression for electrolytes)
II = MRT ( II = osmotic pressure) - nonelectrolytes (organic compounds)
electrolytes
Il =i MRT
ARRHENIUS EQUATION: In k --E/RT + In A
k- Ae KT (T- Absolute Temperature,
k = rate constant, E.= Activation Energy, A = Frequency factor, R= gas constant)
In(kl/k2) = E/R (1/T2-1/T1) Please use at least 3 significant digits in your calculations.
Summary of Rate Laws for Zero-, First-, and Second-Order Reactions
Zero-Order
First-Order
Second-Order
rate law
rate -k
rate - RJAJ
rate - AA
units of rate constant
Ms
s1
M's-1
integrated rate law
[A] = -kt + [A],
In[A] = -kt + In[A], = kt + ()
plot needed for inear ft of rate data
JAl ve. I
nA va.
vs. t
relationship between slope of linear plot and rate
k- -slope
k- -slope
k= slope
constant
half-ite
fa =
f =
The reaction 2 N2Os + 2 N204 + O2 has a rate constant k= 0.055 min. If the
initial concentration of N2Os is 0.980 M, what will be the concentration of N2Os
after 10 minutes?ss
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