Question

A 600 ml sample of nitrogen is heated from 27 ° C to 77 °C at constant

pressure. what is the final volume ?​

Answer 1

Given :

Initial volume (V₁) = 600 ml

Initial Temperature (T₁) = 27°C = 300 K

Final Temperature (T₂) = 77°C = 350 K

To Find :

Final temperature (T₂)

Solution :

As per Charles' Law, At constant pressure a fixed volume of all gases would expand by the same amount for an equal rise in temperature.

    Volume (V) ∝ Temperature (T)

So,

      $\frac{V_1}{T_1}$     =   $\frac{V_2}{T_2}$

⇒   $\frac{600}{300}$     =   $\frac{V_2}{350}$

⇒    V₂    = 350 × 2

∴     V₂    = 700 ml

Hence, the final volume of nitrogen is found to be 700 ml.

Answer 2

Answer:

Concept:

The ideal gas law, in which the pressure of a gas is constant, is a specific case of Charles' law. Charles' law states that the relationship between an absolute gas's volume and temperature is inverse. As long as the gas's pressure and volume remain constant, doubling its temperature causes a gas's volume to double.

Given:

At constant pressure, a 600 ml sample containing nitrogen is heated from 27 °C to 77 °C. Which volume is the last one?

Find:

Find the answer for the given question

Answer:

Changing all temperatures to absolute temperatures should be the initial step in solving difficulties involving the gas law. In other words, convert the temperature to Kelvin if it is supplied in Celsius or Fahrenheit.

$T K = 273 +$ °$C$

$Ti = initial$ $temperature = 27$ °$C$

$Ti$ $K = 273 + 27$

$Ti$ $K = 300 K$

$Tf = final$ $temperature = 77$°$C$

$Tf$ $K = 273 + 77$

$Tf$ $K = 350 K$

Charles' law is expressed as:

$\frac{Vi}{Ti} =\frac{Vf}{Tf}$

where

Vi and Ti represent the initial volume and temperature.

The final volume and temperature are Vf and Tf.

The Vf equation must be solved.

$Vf=\frac{ViTf}{Ti}$

$Vf=\frac{(600ml)(350K)}{(300K)}$

$Vf=700ml$

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