Question
2. A mixture of 4.5% H_(2),76% O_(2). and 19.5% N_(2) has a total pressure of 2.3 atm. What is the partial pressure of each of the gases?
Answer
4.7
(300 Votes)
Hazel
Elite · Tutor for 8 years
Answer
(1) Partial pressure of H2 = 2.3 × (4.5/100) = 0.1035 atm(2) Partial pressure of O2 = 2.3 × (76/100) = 1.748 atm(3) Partial pressure of N2 = 2.3 × (19.5/100) = 0.4485 atm
Explanation
To calculate the partial pressure of each gas, we must first understand the fractional representation of each gas in the mixture. For each gas, the partial pressure is the total pressure of the gas mixture multiplied by the fraction of this specific gas, which itself represents its abundance in the mixture. This technique of calculating partial pressures is based on Dalton's law of partial pressures which explains that the total pressure of a gas mixture can be calculated as the sum of the partial pressures of the composing gases.According to the problem, (1) For hydrogen (H2), the fractional representation = 4.5%(2) For oxygen (O2), the fractional representation is = 76%(4) For nitrogen (N2), the fractional representation is = 19.5%The total pressure is 2.3 atm, hence the partial pressure of each gas would be calculated as:(1) Partial Pressure of H2 = Total pressure × (fraction of H2/100)(2) Partial Pressure of O2 = Total pressure × (fraction of O2/100)(3) Partial Pressure of N2 = Total pressure × (fraction of N2/100)