Question

A five litre flask containing 3.5gr of N2 and 8gr of O2 at 27 degree Celsius. The total pressure exerted by the mixture of these gases

Answer 1

Explanation:

Given A five litre flask containing 3.5 g of N2 and 8g of O2 at 27 degree Celsius. The total pressure exerted by the mixture of these gases

• So Moles of nitrogen n(N2) = 3.5 / 28
•                               So n(N2) = 0.125 mol
• Moles of hydrogen n(h2) = 3 / 2
•                                          = 1.5 mol
• Moles of oxygen n(O2) = 8 / 32
•                                      = 0.25 mol
• Total number of moles of gases n = 0.125 + 1.5 + 0.25
•                                        Or n = 1.875 mol
• We know that total pressure PV = nRT
•                                        Or P = nRT / V
•                                          P = 1.875 x 8.314 x 300 / 5 x 10^-3
•                                  Or P = 9.35 x 10^5 Pa
• Partial pressure of oxygen will be
• P (O2) = P x n(O2) / n
• P(O2) = 9.35 x 10^5 x 0.25 / 1.875

P(O2) = 1.24 x 10^5 Pa

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