Question

: A Ne gas sample has a pressure of 1.20 atm and volume of 35.6 L at 27.0ºC. What is the sample volume if the pressure changes to 3.60 atm and the temperature to 77.0ºC?

Answer 1

Answer:

13.84 L of Ne gas

Explanation:

The exercise can be resolved by applying the General Gas Law, which establishes the relationship between the Pressure, Volume and Temperature of a gas in its initial state and its final state. Mathematically, it is:

$\frac{P1 x V1}{T1} = \frac{P2 x V2}{T2}$

To use this equation, you need to convert the temperatures from Celsius scale to Kelvin scale (absolute scale), and to make this conversion the formula is used:

T (K) = t (° C) + 273.15

We replace the values ​​and obtain the absolute temperatures of the initial state (T₁) and the final state (T₂)

T₁ (K) = 27.0 ° C + 273.15 = 300.15 K

T₂ (k) = 77.0 ° C + 273.15 = 350.15 K

Clearing in the equation of the general gas law V₂, and replacing the other values ​​provided by the statement, the equation and result would be:

$V2 = \frac{P1 x V1 x T2}{T1 x P2} = \frac{1.20atm x 35.6L x 350.5K}{300.15K x 3.60 atm} = 13.84L$

Therefore, the final volume occupied by the gas sample Ne is 13.84 L