Question
In: Chemistry
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.
Solutions
Expert Solution
1. Observe experiments 1 and 2. The initial concentration of A doubles while the initial concentration of B remains constant. As a result, the rate also doubles from 40 mol/L s to 80 mol/L.s. Therefore the reaction is first order with respect to A.
2. Now examine experiments 1 and 3. The initial concentration of A remains constant while concentration of B is doubled from exp. 3 to 1. The result of this change is that the rate of the reaction does not change it remains same. We conclude that B is not a part of the rate law expression.
Therefore, the rate law for the above reaction is:
rate = k [A]
queen_honey_blossom answered 1 year agoRelated Solutions
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
A student is trying to determine the rate law for a reaction involving 2 reactants, A, B and C using the Method of Initial Rates.
I'm stuck on this homework and don't know where to start!
A student is trying to determine the rate law for a reaction
involving 2 reactants, A, B and C using the Method of Initial
Rates. The following initial rate data were obtained at 25 degrees
C. (Note: the overall stoichiometry of the reaction is: A + B + 2C
-> 3 D)
Experiment______Initial [A]______Initial [B]______Initial
[C]_______Initial Rate of Reaction
1______________ 0.1 M_________ 0.1 M_________ 0.2 M
_________4x10^-4 M/min
2_______________...
Using the given data, determine the rate constant of this reaction. A + 2B --> C...
Using the given data, determine the rate constant of this
reaction.
A + 2B --> C + D
Given Data:
Trial [A](M) [B](M) RATE (M/s)
1 .230 .330 0.0231
2 .230 .660 0.0231
3 .460 .330 0.0924
k=? the units are M-1 s-1
Using the given data, determine the rate constant of this reaction. A+2B---> C+D Trial (A) (B)(M)...
Using the given data, determine the rate constant of this
reaction.
A+2B---> C+D
Trial
(A)
(B)(M)
Rate (M/s)
1
0.380
0.330
0.0153
2
0.380
0.660
0.153
3
0.760
0.330
0.0612
k=
(inculde units)
The rate law for the reaction below is given by Rate = k(P ). At 680°C,...
The rate law for the reaction below is given by Rate = k(P ). At
680°C, the half-life is 35.0 s. Given initial pressures of P = 0.67
atm, P = 0.75 atm, and P = 0.25 atm, how many seconds will it take
for the pressure of PH to drop to 0.50 atm
4 PH (g) → P (g) + 6 H (g)
Using the data listed below, determine the rate law and the rate constant for this reaction...
Using the data listed below, determine the rate law and the rate
constant for this reaction at 60°C with respect to hypochlorite
decomposition.
t (min)
[ClO-] (M)
0
0.950
60
0.941
120
0.932
240
0.915
360
0.898
480
0.882
720
0.851
1080
0.809
1440
0.771
1800
0.736
2160
0.705
2520
0.676
2880
0.649
3600
0.601
4320
0.560
5040
0.524
5760
0.493
6480
0.465
7200
0.440
For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
For the reaction A+B+C→D+EA+B+C→D+E, the initial reaction rate
was measured for various initial concentrations of reactants. The
following data were collected:
Trial
[A][A]
(MM)
[B][B]
(MM)
[C][C]
(MM)
Initial rate
(M/sM/s)
1
0.30
0.30
0.30
9.0×10−5
2
0.30
0.30
0.90
2.7×10−4
3
0.60
0.30
0.30
3.6×10−4
4
0.60
0.60
0.30
3.6×10−4
Rate law equation
The rate of a chemical reaction depends on the concentrations of
the reactants. For the general reaction between AA and BB,
aA+bB⇌cC+dDaA+bB⇌cC+dD
The dependence of the...
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
For the reaction A+B+C→D+E, the initial reaction rate was
measured for various initial concentrations of reactants. The
following data were collected: Trial [A] (M) [B] (M) [C] (M)
Initial rate (M/s) 1 0.50 0.50 0.50 1.5×10−4 2 0.50 0.50 1.50
4.5×10−4 3 1.00 0.50 0.50 6.0×10−4 4 1.00 1.00 0.50 6.0×10−4 Rate
law equation The rate of a chemical reaction depends on the
concentrations of the reactants. For the general reaction between
Aand B, aA+bB⇌cC+dD The dependence of the reaction...
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