A 1.50 mol sample of He occupies a volume of 2.50 L at a pressure of 14.7 atm. What will be the pressure of a 1.50 mol sample of H2 gas under the same conditions

14.7 atm

Explanation:

Using the ideal gas law also called the general gas equation ;

PV = nRT

Where,

P = pressure

V = Volume

n = amount of substance

R = ideal gas constant

T = temperature

For the He sample;

V = 2.5 L

n = 1.5 mol

R = 8.314 J/mol/K or 0.0821 L atm/mol/K

T =?

T = PV/nR

T = 14.7*2.5/(1.5*0.0821)

T = 298.42K

For the H2 sample, since both are under the same condition :

P = nRT/V

P = (1.5*0.0821*298.42) ÷ 2.5

P = 14.7 atm.

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

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