By heating 2 mol of nitrogen gas in a frictionless piston-cylinder, the gas expands at a constant pres- sure of 1 bar from an initial volume of 0.02 m² to a final volume of 0.05 m. the gas temperature correspondingly increases from 300 to 500 k. assuming nitrogen is an ideal gas with a molar heat capacity cp = r (where r is the gas constant), find the amount of heat added and work derived from the gas expansion.

Explanation:

The given data is as follows.

    n = 2,          ,      

    = 300 K ,         = 500 K

     P = 1 bar

Equation for work done will be as follows.

                          W =

                              =

                              = - 3000 J

Hence, formula for heat added is as follows.

                       Q =

Putting given values into the above formula as follows.

                    Q =

                       =

                       = 11639.6 J

Thus, we can conclude that the amount of heat added is 11639.6 J.

idk

explanation:

dasdad

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.