Answered

One mole of nitrogen gas confined within a cylinder by a piston is heated from 0°C to 819°C at 1.00 atm.
(b) What would be the temperature change if the gas were heated using the same amount of energy in a container of fixed volume? (Assume that the specific heat capacity of N₂ is 1.00 J/g·K.)

Answer :

shaikhmohd0119

The change in temperature will be 243.07K

Now ,

  Given

T₁ = 0°C = 273K

T₂ = 819°C = 1092K

Hence,

   ΔT = T₂-T₁

        = 1092K - 273K

        = 819K

Now ,

 we know that ,

Work Done (w) = - nRΔT

Where,

 n = No. of moles of Nitrogen

 R = Universal gas constant = 8.314J/K.mol

Hence,

 w = - 1mol× 8.314J/K.mol × 819 K

     = - 6809.17 J

Hence,

  word done in expansion of gas =  - 6809.17 J

b) Now,

      We know that,

 q= mcΔT

Where,

  q = Heat of the substance =  - 6809.17 J

  c = specific heat

  m =mass of the substance

Now,

m = 28.013g/mol × 1 mol
    = 28.013g

Hence,

  6809.17 = 28.013 × 1 × ΔT

    ΔT = 28.013/ 6809.17

       ΔT = 243.07K

Hence,

Thus from the above conclusion we can say that, Change in temperature is 243.07K .

 

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