Answer:
Total pressure = 6.95 atm
pN2) 4.34 atm
p(Ne) =0.44 atm
p(H2) = 2.18 atm
Explanation:
Step 1: Data given
The N2 sample = 7.0 liter at 3.50 atm
The Ne sample = 2.5 liter at 1.00 atm
The H2 sample = 5.0 L at 2.45 atm
Temperature = 25.0 °C
Concentration = 0.160 mol/L
Step 2: Calculate moles
p*V = n*R*T
n = (p*V)/(R*T)
⇒ n = the number of moles of gas
⇒ V = the volume of gas
⇒ p = the pressure of gas
⇒ R = the gas constant
⇒T = the temperature
n(N2) = (3.50*7.0)/(0.08206*298 K)
n(N2) = 1.00 moles
n(Ne) = (1.00*2.5)/(0.08206*298)
n(Ne) = 0.102 moles
n(H2) = (2.45 * 5.0) / (0.08206*298)
n(H2) = 0.501 moles
Step 3: Calculate mol fraction
Total moles = 1.00 + 0.102 + 0.501 = 1.603 moles
Step 4: Calculate mol fraction
Mol fraction = moles gas / total moles
Mol fraction N2 = 1.00 / 1.603 = 0.624
Mol fraction Ne = 0.102/1.603 = 0.0636
Mol fraction H2 = 0.501 / 1.603 = 0.313
Step 5: Calculate total pressure
Total pressure = 3.50 atm + 1.00 atm + 2.45 atm
Total pressure = 6.95 atm
Step 6: Calculate partial pressure
pN2) = 0.624 * 6.95 = 4.34 atm
p(Ne) = 0.0636 *6.95 =0.44 atm
p(H2) = 0.313 *6.95 = 2.18 atm
