2SO(g) <-> 2SO2(g) + O2(g)
1 answer:
The correct reaction is:
2SO₃(g) ⇄ 2SO₂(g) + O₂(g)
Answer:
D.
Explanation:
The equilibrium is reached when the velocity of the formation of products is equal to the velocity of the formation of the reactants, and it's can be represented by the constant of equilibrium Keq, which depends on the temperature.
For a generic reaction:
aA + bB ⇄ cC + dD Keq =
Then, for the reaction given,
Keq = ([O₂]*[SO₂]²)/[SO₃]²
When more O₂ is injected into the reaction, the equilibrium is disturbed, and to solve this, the O₂ must be consumed. So, the amount of SO₂ will be reduced, the amount of SO₃ will be increased, and the value of Keq must remain constant because there's no change in the temperature.
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Answer:
The volume in the first tank = 0.32
The volume in the second tank = 2.066
The final pressure of the mixture = 203.64 K pa
Explanation:
<u>First Tank </u>
Mass = 2 kg
Pressure = 550 k pa
Temperature = 25 °c = 298 K
Gas constant for nitrogen = 0.297
From the ideal gas equation
P V = m R T
550 × V = 2 × 0.297 × 298
V = 0.32
This is the volume in the first tank.
<u>Second tank</u>
Mass = 4 kg
Pressure = 150 K pa
Temperature = 25 °c = 298 K
Gas constant for oxygen = 0.26
From the ideal gas equation
P V = m R T
150 × V = 4 × 0.26 × 298
V = 2.066
This is the volume in the second tank.
This is the iso thermal mixing. i.e.
----- (1)
Put this value in equation (1)
× 2.386 = 550 × 0.32 + 150 × 2.066
= 203.64 K pa
Therefore the final pressure of the mixture = 203.64 K pa