1.5 mol sample he occupies a volume of 2.5 L at a pressure of 14.7 atm what will be the pressure of a 1.5 mol sample of h2 gas under the same conditions

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