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 22 mmHg and a volume of 4.40 L at 34 °C, how many grams of CO2 were used?

a) 0.678 g
b) 1.237 g
c) 2.154 g
d) 3.765 g

Answer 1

To find the number of grams of CO2 used, use the ideal gas law equation PV = nRT. Convert the given temperature to Kelvin and rearrange the equation to solve for the number of moles. Finally, use the molar mass of CO2 to find the number of grams.

Step-by-step explanation:

To find the number of grams of CO2 used, we need to use the ideal gas law equation: PV = nRT, where P represents the pressure, V represents the volume, n represents the number of moles, R represents the ideal gas constant, and T represents the temperature in Kelvin.

To convert the given temperature of 34 °C to Kelvin, we add 273.15 to it, which gives us 307.15 K. Now we can rearrange the equation to solve for the number of moles, n:

n = PV / RT

Plugging in the values from the question, we have:

n = (22 mmHg * 4.40 L) / (0.0821 L.atm/mol.K * 307.15 K)

Solving this equation gives us the number of moles of CO2. To find the number of grams, we can use the molar mass of CO2, which is approximately 44 g/mol. So, the number of grams of CO2 used is:

grams = moles * molar mass

Calculating the value gives us the answer.