A student constructs an electrochemical cell. A diagram of the operating cell and the unbalanced ionic equation representing the
1 answer:
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Answer:
0.008945 atm
Explanation:
In the reaction:
2H2S(g) ⇌ 2 H2(g) + S2(g)
Kp is defined as:
<em>Where P is the pressure of each compound in equilibrium.</em>
If initial pressure of H2S is 3.00atm, concentrations in equilibrium are:
H2S = 3.00 atm - 2X
H2 = 2X
S2: = X
Replacing:
0 = 4X³ - 1.28x10⁻⁶X² + 1.92x10⁻⁶X - 2.88x10⁻⁶
Solving for X:
X = 0.008945 atm
As in equilibrium, pressure of S2 is X, <em>pressure is 0.008945 atm</em>
Answer:
Δ
Δ
Explanation:
Hello,
At the first state, the molar volume is:
The volume in both the second and third state:
Now, as it is about an adiabatic process, one remembers the following relationships:
- Next, for the aforesaid volumes and the first pressure, one computes the second pressure as:
- And the temperature:
- Q:
It is clear that the heat for the first process is 0 as it is adiabatic, but for the second one, it is computed as:
Then the total heat:
- The work for the first process is:
It is clear that the second process is isochoric, so the work here is zero, thus, the total work is:
- For the two processes, ΔU becomes the same value since the system returns to the initial temperature, so ΔU total is 0, thus, for each process, one's got:
- Finally, the total enthapy is also 0 due to same aforesaid reason, thus, each enthalpy is:
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