An ideal gas at 0∘c consists of 1.0×1023 atoms. 20 j of thermal energy are added to the gas. part a what is the new temperature in ∘c?

New temperature T2 = 9.66°C

Explanation:

Given;

Energy added ∆E = 20J

Initial temperature T1 = 0°C

Number of atom = 1.0×10^23

Using the energy equation.

∆E = (3/2)nR∆T

∆T = (2/3)∆E/nR

Where ;

R = universal gas constant = 8.314J/mol-K

n = number of moles = N/Nt

Nt = number of atoms in one mole of gas = 6.022×10^23

n = 1.0 ×10^23/6.022×10^23= 0.166

∆T = (2/3)×20/(0.166×8.314)

∆T = 9.66

T2 = T1+∆T = 0 + 9.66

T2 = 9.66°C

explanation:

considering the bohr theory, the type of connection that requires the transfer the answer conuldn't be right