Question

Using the initial rates of reaction for the following reaction:

A + 3B → 2C

[A] (mol/L) |
[B] (mol/L) |
Initial Rate (mol/L∙s) |

0.210 |
0.150 |
3.41x10 |

0.210 |
0.300 |
1.36x10 |

0.420 |
0.300 |
2.73x10 |

What is the order of the reaction with respect to A?

What is the order of the reaction with respect to B?

The overall rate expression?___________________

Calculate the rate constant including the units.

Answer #1

Rate law = k [ A]^{m} [B]^{n}

K is rate constant , m and n are the order.

Lets find order by using different experimental runs.

Exp No. |
[A] (mol/L) |
[B] (mol/L) |
Initial Rate (mol/L∙s) |

1 |
0.210 |
0.150 |
3.41x10 |

2 |
0.210 |
0.300 |
1.36x10 |

3 |
0.420 |
0.300 |
2.73x10 |

Lets take ratio of rate of exp 3:2 , then we will get order with respect A.

2.37 E-2 / 1.36 E-2 = ( .410/0.210)^{m}

Lets find value of m

m = 1

so the order with respect to A is 1.

To get order with respect to B and for that we use ratio with 2 : 1 .

1.36 E-2/ 3.41 E-3 = (0.300 / 0.150 )^{n}

Lets calculate n

n = 1.99 = 2

order with respect to B = 2

so the rate law becomes

Rate= k [A][B]^{2}

Lets use extp 1 to get k

Rate= k [A][B]^{2}

3.41 E-3 = k (0.210)x(0.150)^{2}

**k = 0.72 L mol ^{-1}
sec^{-1}**

For the reaction 2A + B = 2C + , the following data were
measured at 100 C.
Experiement #
Inital [A] (mol/L)
Initial [B] (mol/L)
Initial Rate (mol/L*min)
1
0.300
0.150
3.58 * 10 ^ -3
2
0.500
0.150
6.01 * 10 ^ -3
3
0.300
0.350
1.91* 10 ^ -2
a) What is the order of the reaction?
b) Calculate the rate constant and indicate its units

Write the equilibrium‑constant expression for the reaction
A(s)+3B(l)↽−−⇀2C(aq)+D(aq)A(s)+3B(l)↽−−⇀2C(aq)+D(aq)
in terms of [A],[A], [B],[B], [C],[C], and [D],[D], as
needed.
Note that ?c,Kc, which is sometimes symbolized as ?eq,Keq,
denotes that the equilibrium constant is expressed using molar
concentrations. For this question, ?cKc means the same thing as
?eq.

For the net reaction: 3AB + 2C → 3A + C2B3, the following slow,
first step has been proposed: 2C → C2 What is the rate law
predicted by this step? Enter the overall order only (no units).
What units are associated with the rate constant for this rate law?
Use M for mol/L and time in s.

The following data were obtained at 25C for a reaction:
aA + bB = cC
Initial Concentrations Initial Reaction Rate
Reaction [A] [B] M/s or mol/Ls
1 0.100 M 0.200 M 5.00x10^-4
2 0.150 M 0.200 M 7.50x10^-4
3 0.150 M 0.600 M 6.75x10^-3
What is the order of the reaction with respect to A?
What is the order of the reaction with respect to B?
What is the rate constant, k, for the reaction?

Determining reaction order: the method of initial rates
2C+3D----> E+F
exp
(c)
(d)
Rate (m/s)
1
2
2
10.00
2
6
2
30.00
3
1
1
1.25
4
2
4
80.00
Determine the order with respect to c and d and calculate the
value of k
THe answer is
ANswer: Rate=k(c)^1(D)^3
K=0.675s^-1M-3
But how do you show the work

1. Given the reaction 2A + 3B à C + 4D
the reaction is zeroth order with respect to A and second order
with respect to B. If the concentration of both A and B are doubled
and the temperature remains unchanged, the rate of the reaction
will increase by a factor of what? Why?
2. The
kinetics of the reaction A+B à P were studied. The following data
was collected. What is the rate law for this reaction?
Why?...

A)A + 3B → 2C
[A] / M
Time / s
0.75
0
0.50
15
0.10
30
What is the average rate of the reaction with respect to A over
the first 15 seconds of the reaction in M/s? (Express your answer
as a decimal, not scientific notation and be mindful of significant
figures)
B)At a certain time in a reaction, substance A is disappearing
at a rate of 4.0 x 10−2 M/s, substance B is appearing at
a rate...

The following chemical reaction occurs in a reactor:
A + 3B ? 2C
It is known that such process has a conversion of 20% for
compound A. The reactor’s feed contains 25 wt% of A and 75 wt% of
B, and has a mass flow of 1000 kg/h. The molecular weights for A
and B are 28 and 2, respectively.
a) What is the molecular weight of C?
b) What is the composition (in wt%) of the output stream?

Anila performed the following reactions between oxalic acid
(H2C2O4) and Permanganate ion and
measured the reaction time at a constant temperature:
MnO4-(aq) +
H2C2O4(aq) -->
MnO2(aq) + CO2(g) + (other products)
rate = k[MnO4-]x
[H2C2O4]y
Determination
Initial [MnO4-], mol/L
Initial [H2C2O4], mol/L
Elapsed time (Δt), s
Reaction rate, mol/L·s
1
0.0230
0.120
224
2
0.0230
0.240
111
3
0.0460
0.240
110
a) (3 pts) Calculate the reaction rate of the
determination 2, using reaction rate =
-Δ[MnO4-]/Δt.
b) (3 pts)...

For the reaction 5A + 2G → 2D + 3E, the following initial rates
of reaction were found.
[A]o/M
[G]o/M
Initial Rate of Reaction / (M/s)
0.655
0.471
8.14×10-3
0.218
0.471
3.01×10-4
0.655
0.236
4.07×10-3
Determine the rate law,
R = k [A] ? [G] ?
Determine the overall order of the reaction.
?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 6 minutes ago

asked 7 minutes ago

asked 7 minutes ago

asked 7 minutes ago

asked 16 minutes ago

asked 22 minutes ago

asked 23 minutes ago

asked 25 minutes ago

asked 25 minutes ago

asked 30 minutes ago

asked 32 minutes ago

asked 39 minutes ago