Question

We start with 5.00 moles of an ideal monatomic gas with an initial temperature of 133 ∘C. The gas expands and, in the process, absorbs an amount of heat equal to 1300 J and does an amount of work equal to 2200 J Use R = 8.3145 J/(mol⋅K) for the ideal gas constant.

Answer 1

Given data,
n= 5.00 moles of an ideal monatomic gas

Initial temperature of T₁ = 133 ° C

Amount of heat energy taken (Q) = 1300J
Work done (W) = 2200J
we know the formula from the Thermo Dynamic first law we have
       Q = U + W
        U = Q - W
           =1300J - 2200J = -900J
we know the formula of the internal energy is

  
              
         
               

-900J = (5.0 mol) x (3/2) [8.314 J/mol. K] [T₂ – (133+273)]

T₂ – 406 = -900 / 62.355 = -14.43

T₂ = 391.56 K

T₂ = 391.70- 273 = 118.57 ° C