State where the chemical potential energy released from a reaction is stored
1 answer:
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Answer:
The workdone by both N₂ and neon gas is 49.3 J
The change in internal energy of N₂ and neon gas is 125.6 J and 73.54 J respectively
The heat for N₂ and neon gas is 171.9 J and 122.84 J respectively.
Explanation:
Given that:
number of moles = 0.05 mole
mass of the piston = 30 kg
diameter = 5.00 cm = 0.05 m
Area (A) = πr²
The piston is said to move from 30 cm - 40 cm
So, the change in volume ΔV is calculated as:
Outside the cylinder; the pressure = 101325 Pa
Thus, workdone = PΔV
=
= 19.90 J
The gravitational work
Given that the height (h) = 10 cm = 0.1 m
Then;
The total workdone for both cases is:
The pressure of gas inside the cylinder is determined as:
a). assuming that the gas is N₂.
Thus, the change in internal energy ΔU is given as:
Since ;
ΔU ≅ 125.6 J
The heat Q = ΔU + W
Q = (122.6 + 49.3) J
Q = 171.9 J
b) In Neon gas:
∴
change in internal energy is;
ΔU = 73.54 J
The heat Q = ΔU + W
Q = (73.54 + 49.3) J
Q = 122.84 J
The given question is incomplete, here is a complete question.
At 400 K, this Reaction has
What Is at 400 K for the following reaction?
(A) 8.2 x 10⁻⁴
(B) 2.9 x 10⁻²
(C) 6.7 x 10⁻⁷
(D) 1.6 x 10⁻⁷
Answer : The correct option is, (C)
Explanation :
The given chemical equation follows:
The equilibrium constant for the above equation, .
We need to calculate the equilibrium constant for the following equation of above chemical equation, which is:
,
The equilibrium constant for the doubled reaction will be the square of the initial reaction.
Or, we can say that
If the equation is multiplied by a factor of '2', the equilibrium constant will be the square of the equilibrium constant of initial reaction.
The value of equilibrium constant for the following reaction is:
Hence, the value of equilibrium constant for the following reaction is,