At 304 K, a 9.6 L tank contains 1.9 moles of H2 gas under an unknown pressure in atm. What is the pressure of the gas in the tank? (R = 0.0821 L*atm/mol*K)

The pressure is 4.939 atm

Explanation:

As we know

PV = nRT

where P is the pressure

V is the volume

n is the total number of moles

R is the gas constant

and T is the temperature

Substituting the given values we get -

The pressure is 4.939 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."

your answer would be “dry”