We start with 5.00 moles of an ideal monatomic gas with an initial temperature of 133...

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.

Expert Solution

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

genius_generous answered 2 years ago

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