PROBLEM 5. Anesthetic gas is normally given to a patient when
the room temperature is 20.0°C and the patient's body
temperature is 37.0°C. What would this temperature change
do to 1600 mL of gas if the pressure and mass remains
constant?
Answers
Answer:
The gas laws are a group of physical laws modeling the behavior of gases developed from experimental observations from the 17th century onwards. While many of these laws apply to ‘ideal’ gases in closed systems at standard temperature and pressure (STP), their principles can still be useful in understanding and altering a significant number of physicochemical processes of the body as well as the mechanism of action of drugs (e.g., inhaled anesthetics).[1]
This argument, which combines physics, medicine, physiology, and biology, starts from the assumption that pressure, volume, and temperature are interconnected variables. Indeed, each gas law holds one constant and observes the variation in the other twoClinical Significance
Boyle’s Law
Boyle’s law can be used to describe the effects of altitude on gases in closed cavities within the body, and to calculate the total intra-thoracic gas volume by body plethysmography. As altitude increases, ambient pressure decreases, and therefore, by Boyle’s Law, volume expansion occurs in enclosed spaces. This effect can be demonstrated by observing the expansion of a sealed bag of potato chips on an ascending commercial flight. In one artificial pneumothorax model, a 40 mL pneumothorax increased in volume by up to 16% at 1.5 km (approx. 5000 feet) from sea level,[4] an effect which may prompt thoracostomy before helicopter transfer to prevent transition to a tension pneumothorax. It is estimated that an expansion of up to 30% for a closed volume of gas in the human body, e.g., a bulla, can be expected after ascending from sea level to an altitude of 2.5 km[5] (approx. 8200 feet).
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Answer:
Volume will change to 1692.83ml