The average kinetic energy of a gas when the particles of the gas collide against each other at a constant temperature and volume will not changes.
<h3>What is average kinetic energy?</h3>
The product of half the mass of each gas molecule with the square of root mean square speed is the average kinetic energy of the molecules.
And this average kinetic energy is deirectly proportional to the absolute temperature of the system but in the given question temperature and volume of the gas is constant. So that there is no change in average kinetic energy of molecules when they collide.
Hence no change in the average kinetic energy of a gas takes place.
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Answer:
The value of the equilibrium constant Kc is 5.45
Explanation:
The "Law of Mass Action" states:
"For a reversible reaction in chemical equilibrium at a given temperature, it is true that the product of the concentrations of the products raised to the stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients is a constant."
This constant was called the equilibrium constant. For a reaction:
aA + bB ⇄ cC + dD
the equilibrium constant Kc is:
In this case, the balanced reaction is:
2 H₂S → 2 H₂ + S₂
So, the equilibrium constant Kc is:
The equilibrium concentrations are
- [H₂S] =0.25 M
- [H₂]= 0.88 M
- [S₂]= 0.44M
Replacing in the definition of equilibrium constant:
Solving:
Kc= 5.45
<u><em>The value of the equilibrium constant Kc is 5.45</em></u>
<u><em></em></u>
Answer : The value of rate constant is,
Explanation :
First we have to calculate the rate constant, we use the formula :
Expression for rate law for first order kinetics is given by:
where,
k = rate constant = ?
t = time passed by the sample = 4.84 s
a = initial concentration = 4.17 M
a - x = concentration after time 4.84 s = 3.56 M
Now put all the given values in above equation, we get
Therefore, the value of rate constant is,
Answer:
110.984 ?
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Explanation:
Answer:
[Ar] 3d10 4s2 4p4
Explanation:
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4