Question

A gas mixture used for anesthesia contains 2.83 mol oxygen (O2), and 8.41 mol of nitrous oxide (N2O). The total pressure of the mixture is 192 kPa. What is the partial pressure of N2O? Report your answer with three significant figures.

Answer 1

Answer: 144 kPa

Step-by-step explanation:

To determine the partial pressure of N2O, first determine the mole fraction of N2O in the mixture, then multiply the mole fraction of N2O by the total pressure.

XN2O = nN2O/ ntotal = 8.41 mol / 2.83 mol + 8.41 mol = 0.7482

PN2O=XN2O×Ptotal = 0.7482 × 192 kPa = 143.7 kPa

Rounding the answer to three significant figures, the partial pressure of N2O is 144kPa.

Answer 2

The partial pressure of N2O is 143.6 kPa

Step-by-step explanation:

Step 1: Data given

Moles O2 = 2.83 mol

Moles N2O = 8.41 mol

Total pressure = 192 kPa

Step 2: Calculate total number of moles

Total numberof moles = moles O2 + molesN2O = 2.83 + 8.41 = 11.24 mol

Step 3: Calculate mole fraction of N2O

Mole fraction N2O = mole N2O / Total moles

Mole fraction N2O = 8.41 / 11.24 = 0.748

Step 4: Calculate partial pressure of N2O

pN2O = 0.748 * 192 kPa

pN2O = 143.6 kPa

The partial pressure of N2O is 143.6 kPa