A flask is filled with 13 g of an ideal gas at 27^oC and its temperature is raised to 52^oC. The mass of the gas that has to be released to maintain the temperature of the gas in the flask at 52^oC, the pressure remaining the same is : 

1.0 g

\(PV \propto\) mass of gas x temperature

In this problem, pressure and volume remain constant.

So : \(M_1 T_1 = M_2 T_2\) = constant

\(\frac{M_2}{M_1} = \frac{T_1}{T_2} = \frac{27 + 273}{52 + 273} = \frac{300}{325} = \frac{12}{13}\)

\(M_2 = M_1 \frac{12}{13}\)

\(M_2 = 13* \frac{12}{13}\) = 12 g1 g

i.e. the mass of gas released from the flask : 13 g - 12 g =