The pressure of a 5.2mol sample of C3H8 in a 35.3 L container is measured to be 5.5 atm. What is the temperature of this gas in kelvins?

T° = 453.6 K

Explanation:

Let's apply the Ideal Gases Law to solve the question:

Pressure . Volume = number of moles . R . T°

We replace data:

5.5 atm . 35.3L = 5.2 mol . 0.082 L.atm/mol.K .T°

T° = (5.5 atm . 35.3L) / (5.2 mol . 0.082 L.atm/mol.K)

T° = 453.6 K

The Ideal Gases Law contains the Absolute value of T° (Kelvin degrees)

So the final answer is: 453.6 K

You can also determine this, because the unit of R (Ideal Gases constant)

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