Final answer:
To find the partial pressure of each gas in a mixture given the mole ratio and total pressure, convert the mole ratios to mole fractions, multiply each mole fraction by the total pressure, and use Dalton's law of partial pressures.
Step-by-step explanation:
The mole ratio of the gases provided is 94:4.0:1.5:0.50. To find the partial pressure of each gas, we must first convert these mole ratios to mole fractions, and then multiply each mole fraction by the total pressure. To find the mole fractions, we add up the moles of all gases to get the total moles and then divide the moles of each individual gas by the total moles. This will give us the mole fraction for each gas. Then the partial pressure PA of each gas can be found using the equation PA = XA * Ptot, where XA is the mole fraction of the gas and Ptot is the total pressure.
The total moles would be 94 + 4.0 + 1.5 + 0.50 = 100. The mole fraction for each gas is then as follows:
- Mole fraction of Gas 1: 94/100 = 0.94
- Mole fraction of Gas 2: 4.0/100 = 0.04
- Mole fraction of Gas 3: 1.5/100 = 0.015
- Mole fraction of Gas 4: 0.50/100 = 0.005
Now, multiplying each mole fraction by the total pressure of 1.54 atm, we can calculate the partial pressures:
- Partial pressure of Gas 1: 0.94 * 1.54 atm = 1.4476 atm
- Partial pressure of Gas 2: 0.04 * 1.54 atm = 0.0616 atm
- Partial pressure of Gas 3: 0.015 * 1.54 atm = 0.0231 atm
- Partial pressure of Gas 4: 0.005 * 1.54 atm = 0.0077 atm
The partial pressures were calculated by using Dalton's law of partial pressures, which states that in a mixture of non-reacting gases, the total pressure is equal to the sum of the partial pressures of individual gases.