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.

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

i think   the answer is c hope i'm right