a 5.00 L flask contains 1.00 mol of diatomic nitrogen and 2.00 mol of diatomic h

Question

a 5.00 L flask contains 1.00 mol of diatomic nitrogen and 2.00 mol of diatomic hydrogen gas at 15 degrees celcius. what are the partial pressures of these gases, and what is the total pressure? a 5.00 L flask contains 1.00 mol of diatomic nitrogen and 2.00 mol of diatomic hydrogen gas at 15 degrees celcius. what are the partial pressures of these gases, and what is the total pressure? a 5.00 L flask contains 1.00 mol of diatomic nitrogen and 2.00 mol of diatomic hydrogen gas at 15 degrees celcius. what are the partial pressures of these gases, and what is the total pressure?

Explanation / Answer

we have to use the formula

partial pressure = mole fraction x total pressure

first find the mole fraction

mole fraction of N2 = moles of N2 / moles of N2 + moles of O2

= 1.0 mol / 1.0 mol + 2.0 mol = 1 / 3 = 0.33

mole fraction of H2 = moles of H2 / total moles

= 2 / 2+1 = 2/3 = 0.67

now calculate the total pressure using PV = nRT formula

P = pressure

V = volume in liters = 5.00 L

n = no of moles = 2+1 = 3

R = gas constant = 0.0821 L atm /mol K

T = temperature in kelvin = 273 + 15 = 288 K

P x 5.00 L = 3 mol x 0.0821 L atm /mol K x 288 K

P = 70.9344 / 5

P = 14.18 atm

partial pressure of N2 = mole fraction of N2 x total pressure

= 0.33 x 14.18 atm

= 4.68 atm

partial pressure of O2 = mole fraction of O2 x total pressure

= 0.67 x 14.18 atm

= 9.5 atm

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