The answer to this question is:
The mobility of electrons.
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Answer:
rate = k[A][B] where k = k₂K
Explanation:
Your mechanism is a slow step with a prior equilibrium:
(The arrow in Step 1 should be equilibrium arrows).
1. Write the rate equations:
2. Derive the rate law
Assume k₋₁ ≫ k₂.
Then, in effect, we have an equilibrium that is only slightly disturbed by C slowly reacting to form D.
In an equilibrium, the forward and reverse rates are equal:
k₁[A][B] = k₋₁[C]
[C] = (k₁/k₋₁)[A][B] = K[A][B] (K is the equilibrium constant)
rate = d[D]/dt = k₂[C] = k₂K[A][B] = k[A][B]
The rate law is
rate = k[A][B] where k = k₂K
<u>Answer:</u> The partial pressure of oxygen gas is 57.8 kPa
<u>Explanation:</u>
Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.
To calculate the partial pressure of oxygen gas, we use the law given by Dalton, which is:
We are given:
Total pressure of the tank, = 201.4 kPa
Vapor pressure of helium, = 125.4 kPa
Vapor pressure of carbon dioxide, = 18.2 kPa
Putting values in above equation, we get:
Hence, the partial pressure of oxygen gas is 57.8 kPa
Answer:
Option B. pentan-1-ol
Explanation:
We'll begin by writing the name of the compound.
The name of the compound above is pentylpropanoate.
From the name of the compound and the structure, we can suggest the following equation:
CH3CH2COOH + HOCH2CH2CH2CH2CH3 —> CH3CH2COOCH2CH2CH2CH2CH3 + H2O
Thus,
Propanoic acid + pentan-1-ol —> pentylpropanoate + water.
Therefore, the alcohol used in the reaction is pentan-1-ol
Answer:
8.65 atm
Explanation:
Using ideal law equation;
PV = nRT
Where;
P = pressure (atm)
V = volume (L)
n = number of moles (mol)
R = gas law constant (Latm/molK)
T = temperature (K)
According to the information given in this question;
V = 18.0 L
n = 6.20 moles
R = 0.0821 Latm/molK
T = 33°C = 33 + 273 = 306K
P = ?
Using PV = nRT
P × 18 = 6.20 × 0.0821 × 306
18P = 155.76
P = 155.76/18
P = 8.65 atm