Question

During laparoscopic surgery, carbon dioxide gas is used to expand the abdomen to help create a larger working space.

If 4.40 L of CO₂ gas at 19∘C at 783 mmHg is used, what is the final volume, in liters, of the gas at 35 ∘C and a pressure of 735 mmHg , if the amount of CO₂ remains the same?

Answer 1

According to Charles's Law, the final volume of the gas at 35°C and a pressure of 735 mmHg is 4.65 liters.

Step-by-step explanation:

According to Charles's Law, at constant pressure, the volume of a gas is directly proportional to its temperature in kelvin. To find the final volume, we can use the formula:

V1 / T1 = V2 / T2

Given:

• V1 = 4.40 L (initial volume)
• T1 = 19°C + 273 = 292 K (initial temperature)
• P1 = 783 mmHg (initial pressure)
• T2 = 35°C + 273 = 308 K (final temperature)
• P2 = 735 mmHg (final pressure)

Plugging in the values:

4.40 L / 292 K = V2 / 308 K

V2 = (4.40 L)(308 K) / 292 K = 4.65 L

Therefore, the final volume of the gas at 35°C and a pressure of 735 mmHg is 4.65 liters.