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Question

One mole of an ideal monoatomic gas is heated at a constant pressure from $$0$$ to $$100$$. Then the change in the internal energy of the gas is:
(Given, $$R=8.32J{ mol }^{ -1 }{ K }^{ -1 }$$)


A
0.83×103J
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B
4.6×103J
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C
2.08×103J
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D
1.25×103J
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Solution

The correct option is C $$1.25\times { 10 }^{ 3 }J$$
Given :        $$T_i  = 0 ^oC = 273  K$$              $$T_f =  100 ^oC = 373 K$$            $$n = 1$$
For monoatomic gas            $$C_v  = \dfrac{3R}{2}$$
$$\therefore$$   Change in internal energy of the gas          $$\Delta U = nC_v  \Delta T$$
 
  $$\Delta U =  \dfrac{3R}{2}n  (T_f - T_i)  =  1\times  \dfrac{3}{2} \times 8.314 \times (373-273)$$

$$\implies$$   $$\Delta U = 1.25 \times 10^3$$  $$J$$

Physics

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