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Reaction kinetics
Page 5
Questions (589)
1. For the 1st order reaction whose rate law constant, k, is 1.5x10-3s-1, t½ is
a. 7.7 minutes *** b. 462 minutes c. 6.5 minutes
2 answers
asked by
moon
544 views
Which of the following rate laws is possible for the following two-step reaction?
1) NO(g) + NO(g) N2O2(g); FAST 2) N2O2(g) +
6 answers
asked by
Sophie
2,099 views
the hydrolysis of sucrose is a part of the digestive process. to investigate how strongly the rate depends on our body
3 answers
asked by
Jose
566 views
For a particular reaction, the rate constant is 2.32 ✕ 10−3 M/s at 185°C and 3.70 ✕ 10−3 M/s at 235°C. What is the
2 answers
asked by
Jamie
487 views
The energy of activation for a reaction is 100kj/mol.Presence of catalyst lowers the activation by 75%.What will be the effect
1 answer
asked by
Lalita
479 views
The rate constant is numerically the same for three reactions of first ,second and third order resp. Which reaction should be
2 answers
asked by
Gagan
639 views
I just want to know if it's possible for two reactants to be first order? I checked my work over and over and redid it and both
1 answer
asked by
Aiyana
288 views
Can someone please explain to me how to calculate reaction order with respect to something?
I've read this in my textbook, and I
2 answers
asked by
Aiyana
486 views
If the reaction rate increases by 2.6 when the temperature increases from 20-30 degrees Celsius, what is Ea?
Do we use 2.6 in
2 answers
asked by
ts
475 views
The rate constant for the equation, 2C2F4 → C4F8, is 0.05 M^−1· s^−1. We start with 0.111 mol C2F4 in a 3.00-liter
1 answer
asked by
David
703 views
Is ΔCP for the reaction > 0 or < 0? Would an atmosphere of 20% carbon dioxide, 5% carbon monoxide, and 75% nitrogen oxidize
1 answer
asked by
Joesph
415 views
If it takes 30 seconds for a reactant concentration to decrease from 1.0 M to 0.5 M in a first-order chemical reaction, then
3 answers
asked by
jameson
708 views
The decomposition of ammonia on a platinum surface at 1129 K occurs according to the
following reaction: 2NH3 (g) �¨ N2(g) +
2 answers
asked by
chancy xdicey
603 views
Which of the following terms are present in the rate law?
A. The rate constant, the concentration of the reactants, and the order
1 answer
asked by
Jessie
650 views
A reaction is thought to be second order with respect to the concentration of carbon monoxide. What evidence would support this?
3 answers
asked by
Jackson
1,799 views
A possible reaction for converting methanol to ethanol is:
CO(g) + 2H2(g) + CH3OH(g) -----> C2H5OH(g) + H2O(g) I completed parts
2 answers
asked by
LC
870 views
The irreversible elementary reaction 2A ---+ B takes place in the gas
phase in an isothermal tubular (plug-Jlow) reactor.
4 answers
asked by
Suleiman
1,298 views
variation of the rate constant with temperature for the first order reaction 2N2O(g) = 2N2O4(g) + O2(g) is given in the
3 answers
asked by
chancy
1,096 views
a first order reaction 50% complets in 20 min.how much time will be required for 90% completion?
1 answer
asked by
nisha
431 views
1. The rate constant for a second order reaction has units of L mol^-1 s^-1. What are the units of the frequency factor, A, for
2 answers
asked by
Student
732 views
Based on the data in this table, what would be the value of k at 795 K?
T k 625 1.1 x 10^-4 635 1.5 x 10^-4 645 2.0 x 10^-4 I
1 answer
asked by
Chemistry
431 views
The experiment can be extended to determine the order of reaction m with respect to [OH-] by varying the concentration of
4 answers
asked by
Alexa
709 views
Reaction Rate = -(1/2) [d(H2O2)/dt] = [d(O2)/ dt]
Using 25 mL of a 0.2 M hydrogen peroxide solution, the following results are
1 answer
asked by
Aaron
481 views
How would the addition of hydrogen gas at constant temperature and volume effect rate=k[h2][I2]?
2 answers
asked by
Marissa
841 views
hey so this is for rate law if the first step is the slow step. it is also an equilibrium. I just want to check if this is
1 answer
asked by
help me lol
358 views
iN A LAB, the orders of two reactants, A and B, were determined experimnetally to be 2 and 3 respectively.
a. write the rate law
2 answers
asked by
Sara
1,195 views
what is the significance of calculating the half life of a reaction?
How has the concept of half-life been used to develop the
2 answers
asked by
anonymous.
604 views
Compare the relative reaction rates of 1-bromobutane, 2-bromopropane, and 2-bromomethylpropane under SN1 reaction conditions.
1 answer
asked by
Jesicca
716 views
Compare the relative reaction rates of 1-bromobutane, 2-bromopropane, and 2-bromomethylpropane under SN1 reaction conditions.
1 answer
asked by
Jesicca
491 views
This type of question come in our exams usually that.
If the Reaction P+Q → R + S is described as being of zero order with
3 answers
asked by
Shahab Mirza
502 views
In an ideal gas, if only one molecule in a thousand has enough energy to react, how can all molecules in a reactor be consumed?
M
1 answer
asked by
Nancy
454 views
Still can't figure this one out-- sorry for reposting, this is the last post, if someone has time to review this question and
1 answer
asked by
Nancy
403 views
1. Spectroscopic studies of the reaction of azide ion with the cluster [Ru3(CO)12] in acetone solvent confirmed the occurrence
1 answer
asked by
Jade
411 views
The initial concentration of a reactant in a zero order is 2.5M. calculate the final concentration of the reactant after 80sec
2 answers
asked by
Nathaniel Benson
43 views
Draw a reaction profile for reaction 2N2+O2+heat→2N2O, must include proper labels for each axis, reactants, products,
3 answers
asked by
Karen
754 views
The rate constant for a second order reaction has the value of 2.5 x 10–3 L·mol–1·s–1. If the initial concentration of
5 answers
asked by
Ana
530 views
Why does a higher concentration increase the rate of reaction?
a It lowers the activation energy. b It increases the surface area
3 answers
asked by
dully
64 views
The reaction OH- + NH4+ = H20 + NH3 is kinetically first order in both reactants' concentrations. The rate constant is 2e10 1/M
2 answers
asked by
Anonymous
464 views
I need to find the rate law of a reaction but ive only done so when factors cancel out, this one has all different numbers and
1 answer
asked by
Amanda
420 views
For the fist order reaction A <-> B, calculate the t1/2(half life) and k(rate constant) and also fill in the blanks.
A-Concetrati
3 answers
asked by
Ivan
451 views
For a second order reaction A <--> B, calculate the t1/2 (half life) and the k(constant) and also fill in the blanks.
A
6 answers
asked by
Ivan
537 views
For the fist order reaction A <-> B, calculate the t1/2(half life) and k(rate constant) and also fill in the blanks.
A-Concetrati
5 answers
asked by
Ivan
444 views
How is the oxygen production in 30 seconds related to the rate of the reaction?
2 answers
asked by
kavi
622 views
for a zero order how long will it take for the concentration of reactant tp fall to one eight is original value if it takes 15.5
1 answer
asked by
azul
375 views
can youi fix the grammar
Rate of reaction refers to the speed at which the concentration of reactant converts to a product, the
2 answers
asked by
p
57 views
The rate constant for this first-order reaction is 0.0990 s–1 at 400 °C.
A --> products After how many seconds will 10.0% of
2 answers
asked by
Sam
619 views
In a reaction, if the concentration decreases faster, that means the reaction has a larger rate constant, and a faster reaction,
1 answer
asked by
K
393 views
what is a descriptive title for an experiment consisting of how alka seltzer dissolves if one is crushed and the other one is
3 answers
asked by
loli
502 views
to find out whether the amount of heat(gas)produced will depend on an increase on the concetration of HCL when HCL reacts with
1 answer
asked by
esmah
318 views
design and conduct an investion to find out whether the amount of heat produced will depend on increase on concentration of Hcl
2 answers
asked by
Jossie
485 views
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Parent Categories (13)
Acid-Base Chemistry
Acid-base reactions
Acids and Bases
Chemical Reactions
Chemistry
Enzymes
Equilibrium
Gases
Organic Chemistry
Physical Chemistry
Reactions
Spectroscopy
Thermodynamics