Respuesta :
Answer:
Partial pressure Ar = 0.378 atm
Partial pressure Kr = 0.180 atm
Partial pressure He = 3.776 atm
Total pressure = 4.334 atm
Explanation:
Step 1: Data given
Mass of Ar = 6.32 grams
Molar mass of Ar = 39.95 g/mol
Mass of Kr = 6.32 grams
Molar mass Kr = 83.80 g/mol
Mass of He = 6.32 g/mol
Molar mass of He = 4.00 g/mol
Volume = 10.3 L
Temperature = 27.0 °C
Step 2: Calculate moles
Moles = mass / molar mass
Moles Ar = 6.32 grams / 39.95 g/mol
Moles Ar = 0.158 moles
Moles Kr = 6.32 grams / 83.80 g/mol
Moles Kr = 0.0754 moles
Moles He = 6.32 grams / 4.00 g/mol
Moles He = 1.58 moles
Step 3: Calculate partial pressures
p*V= n*R*T
p(Ar) = (n*R*T)/V
⇒p(Ar) = the partial pressure of Ar gas = TO BE DETERMINED
⇒n= the number of moles of Ar =0.158 moles
⇒R = the gas constant = 0.08206 L*atm/mol*K
⇒T = the temperature = 27 +273 = 300 K
⇒V = the volume = 10.3 L
p(Ar) = (0.158 * 0.08206 * 300) / 10.3
p(Ar) = 0.378 atm
p(Kr) = (n*R*T)/V
⇒p(Kr) = the partial pressure of Kr gas = TO BE DETERMINED
⇒n= the number of moles of Kr =0.0754 moles
⇒R = the gas constant = 0.08206 L*atm/mol*K
⇒T = the temperature = 27 +273 = 300 K
⇒V = the volume = 10.3 L
p(Kr) = (0.0754 * 0.08206 * 300) / 10.3
p(Kr) = 0.180 atm
p(He) = (n*R*T)/V
⇒p(He) = the partial pressure of He gas = TO BE DETERMINED
⇒n= the number of moles of He =1.58 moles
⇒R = the gas constant = 0.08206 L*atm/mol*K
⇒T = the temperature = 27 +273 = 300 K
⇒V = the volume = 10.3 L
p(He) = (1.58 * 0.08206 * 300) / 10.3
p(He) = 3.776 atm
Step 4: Calculate the total pressure
Total pressure = p(Ar) +p(Kr) +p(He)
Total pressure = 0.378 atm + 0.180 atm + 3.776 atm
Total pressure = 4.334 atm
