Achamber of volume 51 cm^3 is filled with 32.4 mol of helium. it is intially at 459.38°c. (a) the gas undergoes isobaric heating to a temperature of 855.6°c. what is the final volume of the gas? (b) after (a) the chamber is isothermally compressed to a volume 25.3cm^3. compute the final pressure of the helium.

Explanation:

The pressure of the gas can be found out as follows

Gas law formula is as follows

PV = nRT

P = nRT / V

= 32.4 X 8.31 X ( 273 + 459.38 ) / 51 X 10⁻⁶

3866.45 X 10⁶ Pa.

The first change is isobaric therefore

V₁ / T₁ = V₂ / T₂

V₂ = V₁ X T₂/ T₁

= 51 X 10⁻⁶ X ( 855.6 +273) / (459.38 +273)

= 78 X 10⁻⁶

78 cm³

After the first operation , the pressure of the gas remains at

= 3866.45 X 10⁶ Pa.

Now volume of the gas changes from 78 cm³ to 25.3 cm³ isothermally so

P₁V₁ = P₂V₂

P₂ = P₁V₁ / V₂

= 3866.45 X 10⁶ X 78 / 25.3

= 11920 X 10⁶ . Pa

the answer to your question is high voltage and high currency

this means that the temperature of both substances will be equal