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23 July, 00:19

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

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  1. 23 July, 01:57
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    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
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