1)Which of the following changes would decrease the rate at which a solid solute dissolves in a liquid solvent? (3 points)
1 answer:
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Answer:
Rate constant for zero-order kinetics: 1, 58 [mg/L.s]
Rate constant for first-order kinetics: 0,05 [1/s]
Explanation:
The reaction order is the relationship between the concentration of species and the rate of the reaction. The rate law is as follows:
where:
- [A] is the concentration of species A,
- x is the order with respect to species A.
- [B] is the concentration of species B,
- y is the order with respect to species B
- k is the rate constant
The concentration time equation gives the concentration of reactants and products as a function of time. To obtain this equation we have to integrate de velocity law:
For the kinetics of zero-order, the rate is apparently independent of the reactant concentration.
<em>Rate Law: rate = k</em>
<em>Concentration-time Equation: [A]=[A]o - kt</em>
where
- k: rate constant [M/s]
- [A]: concentration in the time <em>t</em> [M]
- [A]o: initial concentration [M]
- t: elapsed reaction time [s]
For first-order kinetics, we have:
<em>Rate Law: rate= k[A]</em>
<em>Concentration -Time Equation: ln[A]=ln[A]o - kt</em>
where:
- K: rate constant [1/s]
- ln[A]: natural logarithm of the concentration in the time <em>t </em>[M]
- ln[A]o: natural logarithm of the initial concentration [M]
- t: elapsed reaction time [s]
To solve the problem, wee have the following data:
[A]o = 100 mg/L
[A] = 5 mg/L
t = 1 hour = 60 s
As we don't know the molar mass of the compound A, we can't convert the used concentration unit (mg/L) to molar concentration (M). So we'll solve the problem using mg/L as the concentration unit.
Zero-order kinetics
we use: [A]=[A]o - Kt
we replace the data: 5 = 100 - K (60)
we clear K: K = [100 - 5 ] (mg/L) /60 (s) = 1, 583 [mg/L.s]
First-order kinetics
we use: ln[A]=ln[A]o - Kt
we replace the data: ln(5) = ln(100) - K (60)
we clear K: K = [ln(100) - ln(5)] /60 (s) = 0,05 [1/s]
Answer:
The question is incomplete as some details are missing. Here is the complete question ; A chemist adds 45.0mL of a 0.434M copper(II) sulfate CuSO4 solution to a reaction flask. Calculate the mass in grams of copper(II) sulfate the chemist has added to the flask. Round your answer to 2 significant digits
Explanation:
The step by step explanation is as shown in the attachment
Answer:
1255.4L
Explanation:
Given parameters:
P₁ = 928kpa
T₁ = 129°C
V₁ = 569L
P₂ = 319kpa
T₂ = 32°C
Unknown:
V₂ = ?
Solution:
The combined gas law application to this problem can help us solve it. It is mathematically expressed as;
P, V and T are pressure, volume and temperature
where 1 and 2 are initial and final states.
Now,
take the units to the appropriate ones;
kpa to atm, °C to K
P₂ = 319kpa in atm gives 3.15atm
P₁ = 928kpa gives 9.16atm
T₂ = 32°C gives 273 + 32 = 305K
T₁ = 129°C gives 129 + 273 = 402K
Input the values in the equation and solve for V₂;
V₂ = 1255.4L