Question
In: Chemistry
The initial rate of the reaction of species A and B A + 2 B →...
The initial rate of the reaction of species A and B A + 2 B → C was measured at a temperature of 25 °C for various initial concentrations of A and B. Data are collected in the table. Determine the rate equation from these data. What is the overall order of the reaction? What is the value of the rate constant? (Give the appropriate units of k.)
| Initial Concentrations, mol/L | Initial Rate | ||
| Experiment | [A] | [B] | mol L-1 s-1 |
| 1 | 0.100 | 0.100 | 4.02 x 10-5 |
| 2 | 0.300 | 0.100 | 1.21 x 10-4 |
| 3 | 0.100 | 0.300 | 1.21 x 10-4 |
Solutions
queen_honey_blossom answered 7 months agoRelated Solutions
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...
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
0.30
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
What is the reaction order with respect to A?
What is the reaction order with respect to B?
What is the reaction order with respect to C?
Express your...
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:
What is the value of the rate constant k for this
reaction?
Trial
[A]
(M)
[B]
(M)
[C]
(M)
Initial rate
(M/s)
1
0.10
0.10
0.10
3.0×10−5
2
0.10
0.10
0.30
9.0×10−5
3
0.20
0.10
0.10
1.2×10−4
4
0.20
0.20
0.10
1.2×10−4
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 0.20 0.20 0.20 6.0×10−5 2 0.20 0.20 0.60
1.8×10−4 3 0.40 0.20 0.20 2.4×10−4 4 0.40 0.40 0.20 2.4×10−4 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...
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...
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.
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
Consider the following reaction. 2 A + B −→ P A table of initial rates with...
Consider the following reaction. 2 A + B −→ P A table of initial
rates with initial concentrations of A and B is given below. [A]o
(M) [B]o (M) rate M s 0.2 0.1 1.2 × 10−5 0.4 0.1 2.4 × 10−5 0.4 0.2
9.2 × 10−5 0.1 0.1 6.0 × 10−6 What is the rate expression? (a) r =
k[A] [B]2 (b) r = k[A] [B] (c) r = k[A]2 [B] (d) r = k[A]2 [B]2
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