One mole of a diatomic gas is heated at const | vedclass

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(C) For an ideal gas at constant pressure,Charles's Law states that $ V \propto T $.Since the volume is doubled $( V_2 = 2V_1 )$,the temperature must

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$ 1050 R $

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(C) For an ideal gas at constant pressure,Charles's Law states that $ V \propto T $.Since the volume is doubled $( V_2 = 2V_1 )$,the temperature must also double.The initial temperature is $ T_1 = 27^{\circ}C = 27 + 273 = 300 	ext{ K} $.The final temperature is $ T_2 = 2 	imes 300 	ext{ K} = 600 	ext{ K} $.The change in temperature is $ \Delta T = 600 	ext{ K} - 300 	ext{ K} = 300 	ext{ K} $.For a diatomic gas,the molar heat capacity at constant pressure is $ C_p = \frac{7}{2}R $.The heat added is given by $ Q = n C_p \Delta T $.Substituting the values: $ Q = 1 	imes \frac{7}{2} R 	imes 300 = 1050 R $.

One mole of a diatomic gas is heated at constant pressure starting at $ 27^{\circ}C $. How much energy must be added to the gas as heat to double its volume?

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