# chemistry 2

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Question description

hello i have about 10 homeworks power points the answes to the question is very simple just find the correct answer and highlit it in the slide and submit back to me, some of the files might not go through the first time so will have send them in chat

DoctorDickens
School: Boston College

Attached.

Clicker Questions

Chapter 14

Barbara Mowery
York College

The rate of a reaction can be
increased by
a.
b.
c.
d.

increasing reactant concentrations.
increasing the temperature.
All of the above

Over time, the rate of most
chemical reactions tends to
_______.
a.
b.
c.
d.

increase
decrease
remain constant
oscillate

Consider the reaction
A2 + 3 B2→ 3 AB3. If ΔA is
–0.750 M/min, then ΔB is
a.
b.
c.
d.

–0.750 M/min.
–0.225 M/min.
–0.250 M/min.
2.25 M/min.

If tripling the concentration of
reactant A multiplies the rate
by a factor of nine, the reaction
is _______ order in A.
a.
b.
c.
d.

zeroth
first
second
third

The relationship that allows us
to study changes in
concentration by measuring
the absorption of light is
a.
b.
c.
d.

Rate = k[A][B].
A = εbc.
ln[A] t = –kt + ln[A]0.
t ½ = 0.693/k.

Select the incorrect statement.
a. The exponents in a rate law are
taken from the coefficients in the
balanced reaction.
b. For a first-order reaction, the plot of
ln[A] versus time is linear.
c. For a zero-order reaction, the plot
of [A] versus time is a parabola.
d. The slope of 1/[A] versus time is the
half-life of a first-order reaction.

Reaction: A + B → C + D
Rate = k[A][B]
The overall order of this
reaction is
a.
b.
c.
d.

first.
second.
third.
fourth.

Reaction: W + X → Y + Z
Rate = k[W]
The order of this reaction with
respect to X is
a.
b.
c.
d.

zeroth.
first.
second.
third.

The time required for the
concentration of a reactant to
be reduced to half of its initial
value is called the
a.
b.
c.
d.

midpoint of the reaction.
equivalence point of the reaction.
half-rate of the reaction.
half-life of the reaction.

If k is the rate constant of a
first-order reaction, the half-life
of the reaction is
a.
b.
c.
d.

0.693/k.
0.693k.
k/2.
2k.

The value of the rate constant
(k) for a first-order reaction is
0.010 sec–1. What is the halflife of this reaction?
a.
b.
c.
d.

10 seconds
69 seconds
100 seconds
690 seconds

A + B → products, Rate = k[A],
k = 0.010 sec–1, Initial [A] =
.100 M, Final [A] = .00100 M
How long will this take?
a.
b.
c.
d.

69 seconds
138 seconds
460 seconds
690 seconds

Rate = k[A]2, Initial [A] = 0.100 M,
k = 0.0214 M–1 sec–1
What is the half-life of this secondorder reaction?
a.
b.
c.
d.

69 seconds
138 seconds
460 seconds
690 seconds

Rate = k[A]2, Initial [A] =
0.100 M, k = 0.0214 M–1 sec–1
After 1.00 hour, what is the
concentration of reactant A?
a.
b.
c.
d.

0.0500 M
0.0250 M
0.0189 M
0.0115 M

The minimum energy that a
collision between molecules
must have for a reaction to
occur is called the
a.
b.
c.
d.

initial energy.
internal energy.
external energy.
energy of activation.

At 298 K, k = 1.36  10–7 sec–1.
At 323 K, k = 2.72  10–6 sec–1.
The energy of activation for this
reaction is
a.
b.
c.
d.

100 kJ/mole.
310 kJ/mole.
690 kJ/mole.
1000 kJ/mole.

The rate-determining step is
the _______ step in a reaction
mechanism.
a.
b.
c.
d.

first
last
fastest
slowest

In a reaction mechanism, a
species that is produced in an
early step and consumed in a
later step is called ___.
a.
b.
c.
d.

a byproduct
a catalyst
an intermediate
a reactant

In a reaction mechanism, a
species on the reactant side
initially that is consumed in an
early step and regenerated in
a later step is called ___.
a.
b.
c.
d.

a byproduct
a catalyst
an intermediate
a reactant

the rate of a chemical reaction
because the presence of the
catalyst
a.
b.
c.
d.

increases molecular velocities.
increases molecular collisions.
decreases energy of activation.
All of the above

Attached.

Clicker Questions

Chapter 15

Barbara Mowery
York College

At equilibrium, the rate of the
forward reaction is _______
the rate of the reverse
reaction.
a.
b.
c.
d.

equal to
slower than
faster than
the reverse of

The reaction quotient Q is
usually represented by
a.
b.
c.
d.

[reactants] / [products].
[products] / [reactants].
[reactants]  [products].
[reactants] + [products].

Select the statement that best
describes a system at
equilibrium.
a. The reaction is complete because all
reactants have become products.
b. The reaction has stopped because all of the
catalyst has been used.
c. As soon as product molecules form, other
molecules of product become reactants.
d. The reaction stops when the amounts of
reactants and products reach equilibrium
amounts.

Which reaction quotient
represents the reaction shown?
Co(s) + 2 H+(aq) → Co2+(aq) + H2(g)
a.

b.

c.

d.

If the value of the equilibrium
constant is large, then at
equilibrium mostly _______
will be present.
a.
b.
c.
d.

reactants
products
catalysts
water

If the value of the equilibrium
constant is small, then at
equilibrium mostly _______
will be present.
a.
b.
c.
d.

reactants
products
catalysts
water

Q = the reaction quotient
K = the equilibrium constant
At equilibrium, which is true?
a.
b.
c.
d.

Q>K
Q HClO > HBrO > HIO
HClO > HBrO > HIO > HClO2
HIO > HBrO > HClO > HClO2
HClO2 > HIO > HBrO > HClO

Aqueous metal ions behave
as Lewis acids because they
a. can readily accept electrons in their
vacant d orbitals.
b. can readily donate electron pairs from
their outermost p orbitals.
c. attract electrons from the water
molecules they are dissolved in.
d. are attracted to the electronegative
oxygen atoms in the solvent.

Attached.

Clicker Questions

Chapter 17

Barbara Mowery
York College

saturated aqueous solution of
_______ decreases its
solubility in water.
a.
b.
c.
d.

BaSO4
Li2CO3
PbS
AgBr

Which of the following
mixtures could be used to
prepare an effective buffer
solution?
a.
b.
c.
d.

HCl and KCl
HNO3 and KNO3
HCl and NH4Cl
...

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Anonymous
Thanks, good work

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