Suppose 16.0 g of oxygen (o2) is heated at constant atmospheric pressure from 26.4°c to 111°c. (a) how many moles of oxygen are present? (take the molar mass of oxygen to be 32.0 g/mol) (b) how much energy is transferred to the oxygen as heat? (the molecules rotate but do not oscillate.) (c) what fraction of the heat is used to raise the internal energy of the oxygen?

a)n=0.5 mol

b)n=0.5 mol

c)U/Q=0.714

Explanation:

Given that

Mass of oxygen m= 16 g

Heated from 26.4°C to 111°C

Molar weight M=32 g/mol

a)

Number of mole,n

n=m/M

n=16/32 mol

n=0.5 mol

b)

Heat,Q

Q= n Cp ΔT

As we know that it is diatomic gas so

Cp=(7/2)R

Q=7 R n ΔT/2

Now by putting the values

----1

Q=1230.88 J

We know that internal energy

--------2

From equation 1 and 2

U/Q= 5/7

U/Q=0.714

the answer is false. this is because for ice to melt, it requires latent heat of melting. latent heat means heat energy required to change phase without any increase in temperatures. therefore, the ice will take energy from the environment to melt hence atmospheric temperatures will reduce.