In chemistry, pressure refers to the force per unit area exerted by gas molecules on the walls of the container in which they are enclosed. It is often measured in units of pascals, atmospheres, millimeters of mercury, or pounds per square inch. Pressure is an important variable used to describe the behavior of gases and is related to other gas variables, such as volume and temperature, through the ideal gas law.
To solve this problem, we can use the combined gas law equation:
(P1V1)/T1 = (P2V2)/T2
where:
P1 = original pressure = 624.0 mmHg
V1 = original volume = 225.0 L
T1 = original temperature = 18.0°C + 273.15 = 291.15 K
P2 = new pressure (what we want to find)
V2 = new volume = 175.0 L
T2 = new temperature = -6.50°C + 273.15 = 266.65 K
Substituting the values into the equation, we get:
(624.0 mmHg x 225.0 L)/291.15 K = (P2 x 175.0 L)/266.65 K
Simplifying and solving for P2, we get:
P2 = (624.0 mmHg x 225.0 L x 266.65 K)/(291.15 K x 175.0 L)
P2 = 536.8 mmHg
Therefore, the new pressure of the gas is 536.8 mmHg.
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