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Sagot :
The question is incomplete. The complete question is :
A 100.0 mL flask is filled with 0.065 moles of A and allowed to react to form B according to the reaction below. The following experimental data are obtained for the amount of A as the reaction proceeds. What is the average rate of appearance of B in units of M/s between t = 10 min. and t = 30 min.? Assume that the volume of the flask is constant. A(g) → B(g)
Time 0.0 10.0 20.0 30.0 40.0
Moles of A 0.065 0.051 0.042 0.036 0.031
Solution :
Consider the following reaction as follows :
[tex]$A \rightarrow B$[/tex]
The experiment data is given as follows :
Time (min) : 0.0 10.0 20.0 30.0 40.0
Moles of A : 0.065 0.051 0.042 0.036 0.031
According to the rate of reaction concept, the rate can be expressed as a consumption of the reactant and formation of the product as follows :
Average rate : [tex]$= -\frac{d[A]}{dt} = \frac{d[B]}{dt} $[/tex]
Now we have to calculate the average rate between 10.0 to 30.0 min w.r.t. A as follows :
Rate [tex]$=-\frac{(0.051-0.036) mol \times \frac{1}{0.1 \ L}}{(30.0-10.0) mol \times \frac{60 \ s}{1 \ min}}$[/tex]
[tex]$=\frac{0.15 \ M}{20 \ min \times \frac{60 \ s}{1 \ min}}$[/tex]
[tex]$= 1.25 \times 10^{-4 }\ M/s$[/tex]
Therefore, the rate = [tex]$= 1.3 \times 10^{-4 }\ M/s$[/tex]
A 100.0-mL flask is filled with 0.065 moles of A and allowed to react to form B. Between 10.0 min and 30.0 min, the average rate of appearance of B is 1.3 × 10⁻⁴ M/s.
What is the rate of reaction?
The rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time.
- Step 1: Write the balanced equation.
A(g) → B(g)
- Step 2: Calculate the rate of reaction of A (rate of disappearance of A).
To calculate the rate of disappearance of A (rA) between 10.0 min and 30.0 min, we will use the following expression.
rA = -ΔnA / V. Δt = -(0.036 mol - 0.051 mol)/ (0.1000 L) (30.0 min - 10.0 min)
rA = 7.5 × 10⁻³ M/min
where,
- ΔnA is the change in the number of moles of A.
- Δt is the change in time.
- Step 3: Calculate the rate of reaction of B (rate of appearance of B).
The molar ratio of A to B is 1:1.
7.5 × 10⁻³ mol A/L.min × 1 mol B/1 mol A = 7.5 × 10⁻³ mol B/L.min
- Step 4: Convert 7.5 × 10⁻³ M/min to M/s
We will use the conversion factor 1 min = 60 s.
7.5 × 10⁻³ M/min × 1 min/60 s = 1.3 × 10⁻⁴ M/s
A 100.0-mL flask is filled with 0.065 moles of A and allowed to react to form B. Between 10.0 min and 30.0 min, the average rate of appearance of B is 1.3 × 10⁻⁴ M/s.
The question is incomplete. The complete question is:
A 100.0 mL flask is filled with 0.065 moles of A and allowed to react to form B according to the reaction below. The following experimental data are obtained for the amount of A as the reaction proceeds. What is the average rate of appearance of B in units of M/s between t = 10 min. and t = 30 min.? Assume that the volume of the flask is constant. A(g) → B(g)
Time (min) 0.0 10.0 20.0 30.0 40.0
Moles of A 0.065 0.051 0.042 0.036 0.031
Learn more about rates of reaction here: https://brainly.com/question/24795637
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