4g argon (Atomic mass =40) in a bulb at a temperature of TK has a pressure P atm. When the bulb was placed in a hot bath at a temperature of 50 degrees C more than the first one, 0.8g of gas had to be removed to get the original pressure. T is equal to :

PV=nRT Consider argon P×V=4/40×R×T We know that molecular weight of Ar=40, On heating, P×V= (3.2/40)*R*(T+50) 4T=3.2T+160 T=160/0.8 =200K

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