Heat is supplied to a sample of a monatomic ideal gas at 40 °C. It is observed that the gas expands until its volume is doubled and the pressure drops to half of its original value. What is the final temperature of the gas?

 40 °C.        

Explanation:

Given that

Initial temperature ,T=40 + 273 = 313 K

Initial pressure = P₁

Initial volume = V₁

Final volume = V₂ = 2 V₁

Final pressure =P₂

Lets take final temperature = T₂

We know that ideal gas equation

P V= m RT

Where ,P=Pressure ,V=Volume ,m=mass ,R=Gas constant , = Temperature

By using mass conservation

Now by putting the values in the above equation we get

Therefore the final temperature will be 313 K or 40 °C.

absorption lines are where light has been absorbed by the atom thus you see a dip in the spectrum whereas.

emission spectra have spikes in the spectra due to atoms releasing photons at those wavelengths.

explanation: