Question

The gas from a certain volcano had the following composition in mole percent: 65% CO2, 25% H2, 5.4% HCl, 2.8% HF, 1.7 % SO2 and 0.1% H2S. What would be the partial pressure of each of these gases if the total pressure the volcanic gas was 760 mmHg?

Answer 1

CO2 = 494 mmHg

H2 = 190 mmHg

HCl = 41.04 mmHg

HF = 21.28 mmHg

SO2 = 12.92

H2S = 0.76 mmHg

Step-by-step explanation

Given:

Composition in mole percent of the gases are:

65% CO2, 25% H2, 5.4% HCl, 2.8% HF, 1.7 % SO2 and 0.1% H2S.

The total pressure of the volcanic gas = 760 mmHg

What to find:

The partial pressure of each of these gases.

Solution:

The partial pressure of each of the gases can be calculated using the % composition and the total pressure.

For 65% CO2

Its partial pressure = (65/100) x 760 mmHg = 494 mmHg

For 25% H2

Its partial pressure = (25/100) x 760 mmHg = 190 mmHg

For 5.4% HCl

Its partial pressure = (5.4/100) x 760 mmHg = 41.04 mmHg

For 2.8% HF2

Its partial pressure = (2.8/100) x 760 mmHg = 21.28 mmHg

For 1.7% SO2

Its partial pressure = (1.7/100) x 760 mmHg = 12.92 mmHg

For 0.1% H2S

Its partial pressure = (0.1/100) x 760 mmHg = 0.76 mmHg