Answer:
Under the same conditions, the pressure of a 1.5 mol H2 sample is 14.7 atm
Explanation:
Step 1: Data given
Number of moles He = 1.5 moles
Volume = 2.5 L
Pressure of the He sample = 14.7 atm
Step 2: Calculate pressure of H2 gas
p(He) * V(He) = n(He) *R*T
⇒Pressure of Helium gas = 14.7 atm
⇒ Volume of the helium sample = 2.5L
⇒ The number of moles He = 1.5 moles
⇒R = the gas constant = 0.08206 L*atm/mol*K
⇒T = The temperature
p(H2) * V(H2) = n(H2) *R*T
Since the conditions are the same:
-Volume of both samples is 2.5L
- Temperature for both is the same
- the gas constant for both is the same (constant)
- The number of moles for both samples is 1.5 moles
Since all the factor are the same, the pressure will also be the same = 14.7 atm
⇒ Volume of the h2 sample = 2.5L
⇒ The number of moles H2 = 1.5 moles
⇒R = the gas constant = 0.08206 L*atm/mol*K
⇒T = The temperature = same temperature
⇒Pressure of H2 gas = 14.7 atm
Under the same conditions, the pressure of a 1.5 mol H2 sample is 14.7 atm
