When a gas is cooled the particles is moving fast or slowly
1 answer:
You might be interested in
Answer: There are 3.2 moles of gas if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature.
Explanation:
Given: Volume = 38.0 L
Pressure = 1430 mm Hg (1 mm Hg = 0.00131579 atm) = 1.9 atm
Temperature = 273.15 K
Using ideal gas equation, the moles of gas will be calculated as follows.
where,
P = pressure
V = volume
n = no. of moles
R = gas constant = 0.0821 L atm/mol K
T =temperature
Substitute the values into above formula as follows.
Thus, we can conclude that there are 3.2 moles of gas if you have a volume of 38.0 L under a pressure of 1430 mmHg at standard temperature.
Answer : The concentration of at equilibrium are 0.132 M, 0.232 M and 0.168 M respectively.
Explanation :
The given chemical reaction is,
First we have to calculate the equilibrium constant for the reaction.
The relation between the equilibrium constant and standard free‑energy is:
where,
= standard free‑energy change = -4.20 kJ/mole
R = universal gas constant = 8.314 J/mole.K
k = equilibrium constant = ?
T = temperature =
Now put all the given values in the above relation, we get:
Now we have to calculate the concentrations of A, B, and C at equilibrium.
The given equilibrium reaction is,
Initially 0.30 0.40 0
At equilibrium (0.30-x) (0.40-x) x
The expression of equilibrium constant will be,
By solving the term x, we get
From the values of 'x' we conclude that, x = 0.716 can not more than initial concentration. So, the value of 'x' which is equal to 0.716 is not consider.
The value of x will be, 0.168 M
The concentration of at equilibrium = (0.30-x) = 0.30 - 0.168 = 0.132 M
The concentration of at equilibrium = (0.40-x) = 0.40 - 0.168 = 0.232 M
The concentration of at equilibrium = x = 0.168 M