Question
In: Chemistry
Some measurements of the initial rate of a certain reaction are given in the table below....
Some measurements of the initial rate of a certain reaction are given in the table below.
|
N2 |
H2 |
initial rate of reaction |
|---|---|---|
|
1.07M |
2.15M |
/17.0Ms |
|
1.07M |
0.951M |
/7.52Ms |
|
4.35M |
2.15M |
/281.Ms |
Use this information to write a rate law for this reaction, and calculate the value of the rate constant.
Round your value for the rate constant to 3 significant figures
Also be sure your answer has the correct unit symbol.
Rate = k?
k = ?
Solutions
queen_honey_blossom answered 8 months agoRelated Solutions
Initial rate data at 25o C are listed in the table below for the reaction: 2NO(g)...
Initial rate data at 25o C are listed in the table
below for the reaction:
2NO(g) + Cl2(g) → 2NOCl(g)
[NO]i (M)
[Cl2]i(M)
Initial rate (M/s)
0.13
0.20
1.0 x 10-2
0.26
0.20
4.0 x 10-2
0.13
0.10
5.0 x 10-3
First determine the experimental rate law and calculate the the
value of the rate constant, k (no units).
k =
Tries 0/45
Then, calculate the initial rate of this reaction, when the
initial concentration of NO is 0.78 M...
Consider this initial-rate data at a certain temperature for the reaction described by :  
Consider this initial-rate data at a certain temperature for the
reaction described by
:
OH-(aq)
OCl-(aq) + I- (aq) --------------> OI-(aq) + Cl-(aq)
Trial [OCl-]0
(M)
[I-]0
(M)
[OH-]0
(M)
Initial rated (M/s)
1
0.00161
0.00161
0.530
0.000335
2
0.00161
0.00301
0.530
0.000626
3
0.00279 0.00161
0.710
0.000433
4
0.00161
0.00301
0.880
0.000377
Determine the tate law and the value of the rate constant for
this reaction.
A) What is the Hrxno in (kJ) for the reaction below, given the relevant table on...
A) What is the Hrxno in (kJ) for the
reaction below, given the relevant table on the info sheet. PbO(s)
+ 2HBr(g) ---> PbBr2(s)+H2O(g).
a) -273
b) -229
c) -265
d) Not enough information provided.
B. What is the Hrxno in (kJ) for
2PbBr2(s) + 2H2O(g) ---> 2PbO(s) +4HBr(g)
using the thermochemical equation in part A.
a) 545
b) 530
c) 458
d) 229
The rate of a certain reaction was studied at various temperatures. The table shows temperature (T)...
The rate of a certain reaction was studied at various temperatures. The table shows temperature (T) and rate constant (k) data collected during the experiments. Plot the data, and then answer the following questions.
What is value of the activation energy, E_a for this reaction
What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction
The rate of a certain reaction was studied at various temperatures. The table shows temperature (T)...
The rate of a certain reaction was studied at various
temperatures. The table shows temperature (T) and rate constant (k)
data collected during the experiments. Plot the data to answer the
questions.
What is the value of the activation energy, Ea , for this
reaction?
T (K)
k (s−1)
400
0.000108
420
0.000626
440
0.00310
460
0.0134
480
0.0511
500
0.175
520
0.547
540
1.57
560
4.18
580
10.4
3. Given the initial rate data for the reaction A + B –––> C, determine the...
3. Given the initial rate data for the reaction A + B –––> C,
determine the rate expression for the reaction. [A], M [B], M Δ
[C]/ Δ t (initial) M/s 0.215 0.150 5.81 x 10–4 0.215 0.300 1.16 x
10–3 0.430 0.150 2.32 x 10–3 A) (Δ[C]/Δt) = 1.80 x 10–2 M –1 s –1
[A][B] B) (Δ[C]/Δt) = 3.60 x 10–2 M –1 s –1 [A][B] C) (Δ[C]/Δt) =
1.20 x 10–1 M –2 s –1 [A][B]2 D)...
Given the initial rate data for the reaction being A + B --> D determine the...
Given the initial rate data for the reaction being A + B -->
D determine the rate expression for the reaction
and the (k) rate constant. (The units of [A] [B]
are moles/liter and the units of IRR is moles/liter seconds).
If the [A]=[B]=.030M, what would the IRR be?
[A]
[B]
IRR
0.020
0.010
.028
0.020
0.020
.224
0.020
0.040
1.792
0.40
0.020
.448
.010
0.020
.056
Given the initial rate data for the reaction being A + B --> D determine the...
Given the initial rate data for the reaction being A + B -->
D determine the rate expression for the reaction
and the (k) rate constant. (The units of [A] [B]
are moles/liter and the units of IRR is moles/liter seconds).
If the [A]=[B]=.030M, what would the IRR be?
[A]
[B]
IRR
0.020
0.010
.028
0.020
0.020
.224
0.020
0.040
1.792
0.020
.448
.010
0.020
.056
Determine the rate law for the reaction A+ B → C given the following initial rate data.
Determine the rate law for the reaction A+ B → C given the following initial rate data.
[A], M [ B], M ∆[C]/∆t (mol/L•s)
0.10 0.20 40.
0.20 0.20 80.
0.10 0.10 40.
The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial...
The rate constant for a certain reaction is k = 1.90×10−3 s−1 .
If the initial reactant concentration was 0.850 M, what will the
concentration be after 15.0 minutes? A zero-order reaction has a
constant rate of 2.80×10−4 M/s. If after 75.0 seconds the
concentration has dropped to 9.00×10−2 M, what was the initial
concentration?
A zero-order reaction has a constant rate of
2.80×10−4M/s. If after 75.0 seconds the
concentration has dropped to 9.00×10−2M, what
was the initial concentration?
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