Question

During laparoscopic surgery, carbon dioxide gas is used to expand the abdomen to help create a larger working space.f 4.90 L of CO₂ gas at 17 ∘C at 795 mmHg is used, what is the final volume, in liters, of the gas at 33 ∘C and a pressure of 753 mmHg , if the amount of CO₂ remains the same?

Answer 1

According to Charles's Law, the final volume can be calculated using the equation V1/T1 = V2/T2. Substituting the given values, the final volume is approximately 5.54 L.

Step-by-step explanation:

According to Charles's Law, at constant pressure, the volume of a gas is directly proportional to its temperature. Therefore, we can use the equation V1/T1 = V2/T2 to solve this problem.

Given that the initial volume (V1) is 4.90 L at a temperature (T1) of 17 °C, the final temperature (T2) is 33 °C, and the pressure remains constant, we can substitute these values into the equation and solve for the final volume (V2).

V2 = (V1 x T2) / T1

= (4.90 L x (33 °C + 273.15 K)) / (17 °C + 273.15 K)

≈ 5.54 L