A gas is initially at a pressure of 0.43 atm, and a volume of 11.7 liters. Then the pressure is raised to 3.61 atm and the volum e is decreased to 9.5 liters. This causes the temperature to raise to 627 K. What was the initial temperature of the gas? A. 83.19 K B. 7.32 K C. 327.97 D. 91.98 K
2 answers:
Answer:
D. 91.98K
Explanation:
The General Gas Law equation is given by,
From the question,
the initial pressure,
the initial volume,
the final temperature,
the final pressure,
the final volume,
Making
the subject of the expression, we obtain
By substitution,
Hence the initial temperature was 91.98 K
The Initial temperature was 92.24 K
<h2>Further Explanation;</h2><h3>Boyle's law </h3>
Boyle's law states that the volume of a fixed mass of a gas is inversely proportional to its pressure at a constant temperature. That is;
, where k is a constant
Charles' Law
Charles's law states that the volume of a fixed mass of a gas is directly proportional to absolute temperature at constant pressure. That is; , where k is a constant <h3>Combined gas law</h3>
Combined gas law combines both Boyle's law and Charles's law. It states that the volume of a fixed mass of a gas is directly proportional to absolute temperature and inversely proportional to pressure. That is;
Given;
While;
To calculate
Therefore the initial temperature is 92.24 K
Keywords : Combined gas laws, Boyle's law and Charles's law
<h3>Learn more about:</h3>
Level: High school
Subject: Chemistry
Topic: Gas laws
Sub-topic: Combined gas laws
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