Question

The reaction is 2H202(1) = 2H20(l) + 02(g)

The reaction is second order equation and show all work

How long does it take the solution to decrease by 10% of the original concentration if k = 4.18 x 10^9 at constant temperature

Answer #1

For the reaction
2 NOBr(g)----> 2 NO(g) + Br2(g)
the rate law is second order in NOBr with a rate constant of
8.50 x 10-2 M-1·s-1 at
35°C. If the initial concentration of NOBr is 1.00
M, how many seconds does it take for [NOBr] to
decrease to 0.10 M?
A) 47 seconds
B) 72 seconds
C) 106 seconds
D) 163 seconds
E) 224 seconds
The answer is C (106 seconds) how do you get
this? Please be detailed and...

1)At 25°C, some second-order reaction 3 X
(g)→ 2 Y (g) + Z
(g) has a half-life of 5.82 hours when the
initial concentration of X is 4.46 M.
(a) What is rate constant for this reaction?
(b) How much X will be left after
17.5 hours?
Example of answer: (a)
k = [type
your answer] M–1 h–1;
(b) [X]t =
[type your answer] M.
2)
For some second-order reaction: 3 X
(g)→ Y (g) + Z
(g).
The following...

a reaction that is second-order in one reactant has a
rate constant of 2.2 x 10-2L/ (mol*s) if tbe inital concentration
of the reactant is 0.360 mol/L, how long will it take for the
concentration to become 0.180 mol/L

The deposition of HOF occuras at 25C 2 HOF(g) = 2 HF(g) +02 (g)
I need to show my work and all equations used. I also included the
answers but I do not know how to calculate them
The graph is attached at
https://docs.google.com/document/d/10__3VzL8YDJaqchUPYVmSfhQyH5fYMts9Oj9jMRjs4g/edit?usp=sharing
What is the initial concentration of
HOF? .54
Write
the rate law for this reaction. Include the value and units for the
rate constant. rate .17 1[HOF}
How long will it take for the
concentration...

The reaction in which NO2 forms a dimer is second order in
NO2 :
2NO2(g) ---> N2O4(g) Rate =
k [NO2]2
Calculate the rate constant for this reaction if it takes 0.0050
s for the initial concentration of NO2 to decrease from
0.50M to 0.25M.

Consider the reaction: IO4- (aq) + 2H20 (l) <----> H4IO6-
(aq) If you start with 25.0 mL of a 0.905M solution of NaIO4, and
then dilute it with water to 500.0mL, what is the concentration of
H4IO6- at equilbrium? Assume Kc = 3.5 x 10^-2

The rate constant of a first-order reaction is 0.0032 x
10-4 L/mol *s at 640 K. If the activation energy is
176,406J/mol, calculate the temperature at which is rate constant
is 0.0039 x10 -4 L/mol*s.
Show your work please.

The rate constant for this second-order reaction is 0.120
M^-1·s^-1 at 300 °C. A rightarrow products. How long (in seconds)
would it take for the concentration of A to decrease from 0.880M to
0.300M?

Please show your work!
a) Write the equlibrium equation for the following reaction.
N2 (g) + 3 H2 (g) <===> 2
NH3 (g)
b) An equilibrium mixture at 500 K has the following
concentrations : [N2] = 3.0 x 10-2 M,
[H2] = 3.7 x 10-2 M, [NH3] = 1.6 X
10-2 , calculate the equilibrium constant,
Kc.
c) Calculate the Kp for this reaction.
d) Is the equilibrium mixture mostly reactants or products?
e) Does this reaction go to...

1)A second order reaction has a rate constant of 3.7
M-1min-1. if the initial concentration of the reactant is 0.0100M,
what is the concentration remaining after 15 min?
a) .0099M
b) .0056M
c) .0025M
d) .0064M
2) the rate constant for the first order decomposition
of A at 500 degrees Celsius is 9.2 x 10 to the negative 3rd powers
s-1. How long will it take for 90.8 % of a 0.500M sample of A to
decompose
a) 2.5 x...

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