Ideal Gas Law PV = nRT
1 answer:
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Answer:
e. As equilibrium is reestablished, the partial pressure of hydrogen decreases.
Explanation:
Hello,
In this case, for the given chemical reaction:
Considering the Le Chatelier's principle which states that adding more reactant shifts the reaction towards the products, condition that is related with the doubling of the hydrogen partial pressure, we can notice that e. As equilibrium is reestablished, the partial pressure of hydrogen decreases since the addition of hydrogen will be used to form more methane and hydrogen sulfide, for that reason, its amount is decreased to reattain equilibrium.
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Answer:
Work done in this process = 4053 J
Explanation:
Mass of the gas = 0.092 kg
Pressure is constant = 1 atm = 101325 pa
Initial temperature = 200 K
Final temperature = 200 - 85 = 115 K
Gas constant for nitrogen = 297
When pressure of a gas is constant, volume of the gas is directly proportional to its temperature.
⇒ V ∝ T
⇒ =
------------ ( 1 )
From ideal gas equation
= m R
------ (2)
⇒ 101325 × = 0.092 × 297 × 200
⇒ = 0.054
This is the volume at initial condition.
From equation 1
⇒ =
⇒ = 0.094
This is the volume at final condition.
Thus the work done is given by W = P [ -
]
⇒ W = 101325 × [ 0.094 - 0.054]
⇒ W = 4053 J
This is the work done in that process.
Answer:
The enthalpy of the reaction is 64.9 kJ/mol.
Explanation:
..[1]
..[2]
..[3]
..[4]
2 × [2] - [1]- [3] = [4] (Using Hess's law)
The enthalpy of the reaction is 64.9 kJ/mol.