Avogadro's hypothesis says that 2.0 L of Cl2 (g) occupies the same volume as 2.0 L of CO2. So <span>(2.0L of Cl2 (g)
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I was thinking that the question would be to find for the operating temperature of the reaction. Change in entropy is equal to the total energy divided by the temperature. Assuming it is isothermal, internal energy would be zero. Therefore, the temperature would be:
T = 129000/301 = 428.57 K
Answer:
The temperature above which the reaction be spontaneous is 331.3 K.
Below this temperature; the backward reaction is the favored reaction.
Explanation:
- We have an important relation from the third law of thermodynamics:
<em>ΔG = ΔH - TΔS</em>
<em>ΔG is the free energy change of the reaction,</em>
<em> ΔH is the enthalpy change of the reaction,</em>
<em>ΔS is the entorpy change of the reaction,</em>
- <em>The reaction is spontaneous when ΔG is negative.</em>
- and ΔG be negative when the value of (TΔS) is higher than the value of (ΔH).
<em>When ΔG = 0, ΔH = TΔS.</em>
For this reaction, ΔH = 30.91 KJ and ΔS = 0.0933 KJ/K.
- The temperature above which the reaction be spontaneous is:
T = ΔH / ΔS = (30.91 KJ) / (0.0933 KJ/K) = 331.29 K ≅ 331.3 K.
<em>∴ The temperature above which the reaction be spontaneous is 331.3 K.</em>
<em>Below this temperature; the backward reaction is the favored reaction.</em>
Answer: With the cold front, warm air is rapidly forced upward (like the shavings) in advance of the actual front (the “cutter”), creating towering cumulus clouds, some hard showers and quite possibly a few gusty thunderstorms followed by a push of cooler and drier air in its wake.
Explanation:
