What is the molar mass of a gas which occupies 48.7 l at 111oc under 698 torr of pressure and has a mass of 21.5 grams?

Molar mass of the gas = 15.15 g/mol

Explanation:

PV = nRT

Where,

P = pressure

n = No. of moles

R = Gas constant

T = Temperature

P = 698 torr, 1 torr = 0.00131579 atm

Temperature = 111 °C = 100 + 273.15 = 384.15 K

V = 48.7 L

R = 0.082057 L atm/mol K

Now, PV = nRT

          =1.4189 mol

Molar mass = Mass/ No. of  moles

                    = 21.5/1.4189

                    =15.15 g/mol

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.