What is the pressure of 0.5 mol nitrogen (n2) gas in a 5.0 l container at 203 k?

The pressure of 0.5 mole of nitrogen gas=

Given:

Moles of nitrogen gas=0.5mole

Volume of nitrogen gas=5L

Temperature of nitrogen gas=203K

To Find:

Pressure of 0.5g mole of nitrogen gas

Step by Step by Explanation:

Formula used for calculating the pressure of a gas is achieved through ideal gas equation

According to Ideal Gas;

From this above equation, pressure can be calculated as

Where P=Pressure of the gas

N=number of moles=0.5moles

R=Gas constant

V=Volume of nitrogen gas in litres=5L

T=Temperature of nitrogen gas=203K

Substitute all the values in the above equation we get

Result:

Thus the pressure of 0.5 mole of nitrogen gas is

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml