Agas sample has a volume of 2.0 l at 0.75 atm and 27°c. what temperature (in °c) would be required to increase the volume to 3.0 l at constant pressure?

In the case, the temperature required to increase the volume is 40.5 °C.

Explanation:

Charles Law:

At a constant pressure, the volume of a gas is proportional to its temperature. It is expressed as

V₁ / T₁ = V₂ / T₂   (1)

where V₁ T₁ are initial volume and temperature of the gas and V₂ T₂ are the final volume and temperature of the gas.  

Given data:

V₁ = 2 L

T₁ = 27 °C

V₂ = 3 L

T₂ = ?

Sol:

Using equation (1)

V₁ / T₁ = V₂ / T₂

Rearranging the above equation we get,

T₂ = V₂ x (T₁ / V₁ )

Now Putting the values of  V₁ , T₁ and V₂ in above equation:

T₂ = 3 x (27 / 2)

T₂ = 40.5 °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:

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