Question

Laparoscopic surgery involves inflating the abdomen with carbon dioxide gas to separate the internal organs and the abdominal wall. If the CO2 injected into the abdomen produces a pressure of 17 mmHg and a volume of 4.15 L at 36 °C, how many grams of CO2 were used?

a) 0.935 g
b) 1.365 g
c) 2.265 g
d) 3.850 g

Answer 1

To calculate the mass of CO2 used in laparoscopic surgery, we can use the ideal gas law equation to find the number of moles and then convert them into grams using the molar mass of CO2.

Step-by-step explanation:

Laparoscopic surgery involves inflating the abdomen with carbon dioxide gas to separate the internal organs and the abdominal wall. To calculate the mass of CO2 used, we need to use the ideal gas law equation:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

We need to convert the given temperature from Celsius to Kelvin:

T(K) = T(°C) + 273.15

Substituting the known values and solving for moles:

n = PV / RT

Since we want to find the mass of CO2, we need to convert moles to grams using the molar mass of CO2, which is 44.01 g/mol. Therefore, the number of grams of CO2 used can be calculated as:

mass = n x molar mass