Question

Based on the kinetic data below, what is the rate constant for
this reaction?

A + 2 B => C

[A], mol/L | [B], mol/L | Initial Rate, mol L^{-1} s^{-1} |

1.0 x 10^{-4} |
2.0 x 10^{-4} |
0.276 |

2.0 x 10^{-4} |
1.0 x 10^{-4} |
0.069 |

1.0 x 10^{-4} |
1.0 x 10^{-4} |
0.069 |

Based on the kinetic data below, what is the rate constant for
this reaction?

A + 2 B => C

[A], mol/L | [B], mol/L | Initial Rate, mol L^{-1} s^{-1} |

1.0 x 10^{-4} |
2.0 x 10^{-4} |
0.276 |

2.0 x 10^{-4} |
1.0 x 10^{-4} |
0.069 |

1.0 x 10^{-4} |
1.0 x 10^{-4} |
0.069 |

2.8 x 10^{7} s^{-1} |

6.9 x 10^{6} L mol^{-1} s^{-1} |

3.5 x 10^{6} L mol^{-1} s^{-1} |

6.9 x 10 |

Answer #1

For the reaction, A(g) + B(g) => 2 C(g), the following data
were obtained at constant temperature.
Experiment
Initial [A], mol/L
Initial [B], mol/L
Initial Rate, M/min
1
0.10
0.10
2 x 10-4
2
0.30
0.30
5.4 x 10-3
3
0.10
0.30
1.8 x 10-3
4
0.20
0.40
6.4 x 10-3
Which of the following is the correct rate law for the
reaction?
1.
Rate = k[A][B]
2.
Rate = k[A]2[B]
3.
Rate = k[A]2[B]2
4.
Rate = k[A]
5....

Given the data below for the reaction, 2 A + 2 B + 4 C => D +
E + 3 F,
Experiment
Initial conc of A, mol/L
Initial conc of B, mol/L
Initial conc of C, mol/L
Initial rate, mol/L.s
1
0.1
0.2
0.4
2 x 10-3
2
0.2
0.2
0.4
8 x 10-3
3
0.3
0.4
0.4
1.8 x 10-2
4
0.4
0.6
0.2
1.6 x 10-2
Calculate the value of k to 3 significant figures

The following data were obtained for the chemical reaction: A +
B ---> products
Exp.
Initial A
(mol/L)
Initial B
(mol/L)
Init. Rate of Formation
of products (M s-1)
1
0.040
0.040
9.6 x 10-6
2
0.080
0.040
1.92 x 10-5
3
0.080
0.020
9.6 x 10-6
(a) Determine the rate law for this reaction.
(b) Find the rate constant.
(c) What is the initial rate of reaction when [A]o =
0.12 M and [B]o = 0.015

Using the given data, calculate the rate constant of this
reaction: A+B ---> C+D
Trial
[A] (M) [B}
(M)
Rate (M/s)
1
0.230
0.330
0.0170
2
0.230
0.792
0.0979
3
0.276 0.330
0.0204

The reaction
A → C
was performed and the concentration vs. time data below
collected.
time,
s
0
1
2
3
4
5
6
7
8
[A],
mol/L
0.7905
0.5041
0.3214
0.2049
0.1307
0.08332
0.05313
0.03388
0.02160
Complete the rate law for the reaction by filling in the values
for the rate constant and reaction order.
Rate = k[A]x
rate constant (without units) =
reaction order =

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 the reaction below was determined to be
3.241×10-5 s–1 at 800 K. The activation energy of the reaction is
215 kJ/mol. What would be the value of the rate constant at
9.10×102 K? N2O(g) --> N2(g) + O2(g)
I'm having trouble calculating the rate constant with the
arrhenius equation that deals with two temps, could you show me the
step by step how to do this?

Consider the reaction and the initial concentration and initial
rate data below.
BrO3-(aq) + 5 Br- (aq) + 6 H+(aq) ® 3 Br2 (aq) + 3 H2O (l)
Experiment
[BrO3-], (M)
[Br-],(M)
[H+],(M)
Initial Rate (M/sec)
1
0.10
0.10
0.10
1.2 x 10-3
2
0.20
0.10
0.10
2.4 x 10-3
3
0.10
0.30
0.10
3.5 x 10-3
4
0.20
0.10
0.15
5.4 x 10-3
Determine the rate law for this reaction
What is the overall order of the rate law?...

"For the reaction 2 N2O5 --> 4 NO2 + O2 the rate constant is
6.82 x 10^-3 s^-1 at 70 degrees Celsius. The reaction is first
order overall. If you start with 0.350 mol of dinitrogen pentoxide
in a 2.0 L volume, how many miles will remain after 10 minutes? How
long will it take for you to have 0.125 moles of reactant left?
What is the half-life of dinitrogen pentoxide?"
*Please show all work.
* if it's out of...

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

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