According to Clausius-Clayperon equation,
is the vapor pressure at boiling point = 760 torr
is the vapor pressure at T_{2} =638.43 torr
Temperature
Δ
Plugging in the values, we get
ln
Therefore, the boiling point of octane = 389 K - 273 =
Answer is: A. adding heat to the product mixture.
Balanced chemical reaction:
CO(g) + 3H₂(g) ⇄ CH₄(g) + H₂O(g); ΔH = -206.1 kJ.
This reaction is exothermic, which means that heat is released.
According to Le Chatelier's principle when the reaction is exothermic heat is included as a product and when the temperature increased, the heat of the system increase, so the system consume some of that heat by shifting the equilibrium to the left.
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Answer:</h3>
327° C
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Explanation:</h3>
The initial temperature of the gas is 27°C
We need to find the final temperature.
If we assume the initial pressure is y
The final temperature will be 2y
Using the pressure law;
Therefore,
Therefore, the new temperature is 600 K or 327° C
Answer:
they're close to filling their outer shell, fulfilling the octet rule
Explanation: