Question

4. A gas with a pressure of 5.4 atm and at 25C is raised to a new temperature of 78C.

Answer 1

The answer for the following problem is mentioned below.

• Therefore the final pressure of the gas is 6.3 atm

Explanation:

Given:

Initial pressure ($P_{1}$) = 5.4 atm

Initial temperature ($T_{1}$) = 25°C = 273 + 25 = 298 K

Final temperature ($T_{2}$) = 78°C = 273 + 78 = 351 K

To solve:

Final pressure ($P_{2}$)

We know,

From the ideal gas equation,

P × V = n × R × T

Here from the above equation we can tell that ;

      P ∝ T

So;

we can write as;

  $\frac{P}{T} \f$ = constant

(i.e.)

        $\frac{P_{1} }{P_{2} }$ = $\frac{T_{1} }{T_{2} }$

Where;

$P_{1}$ = Initial pressure of the gas

$P_{2}$ = final pressure of the gas

$T_{1}$ = initial temperature of the gas

$T_{2}$ = final temperature of the gas

              $\frac{5.4}{P_{2} }$  = $\frac{298}{351}$

               $P_{2}$ = $\frac{5.4*351}{298}$

               $P_{2}$ = 6.3 atm

Therefore the final pressure of the gas is 6.3 atm