At 0,^{circ}C temperature and 1, atm pressure | vedclass

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(B) Given: $P_1 = 1\, atm$,$V_1 = 100\, cc$,$T_1 = 0\,^{\circ}C = 273\, K$ $P_2 = 1.5\, atm$ $T_2 = T_1 + \frac{T_1}{3} = 273 + \frac{273}{3} = 273

Vedclass · Accepted Answer

$88.9$

Vedclass · Answer

(B) Given: $P_1 = 1\, atm$,$V_1 = 100\, cc$,$T_1 = 0\,^{\circ}C = 273\, K$ $P_2 = 1.5\, atm$ $T_2 = T_1 + \frac{T_1}{3} = 273 + \frac{273}{3} = 273 	imes \frac{4}{3} = 364\, K$ Using the ideal gas equation: $\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$ $V_2 = \frac{P_1 V_1 T_2}{P_2 T_1} = \frac{1 	imes 100 	imes (273 	imes \frac{4}{3})}{1.5 	imes 273}$ $V_2 = \frac{100 	imes 4}{1.5 	imes 3} = \frac{400}{4.5} = 88.88\, cc \approx 88.9\, cc$

At $0\,^{\circ}C$ temperature and $1\, atm$ pressure,the volume of a gas is $100\, cc$. If the pressure is increased by $1.5$ times and the temperature is increased by one-third of its absolute temperature,what will be the final volume of the gas in $cc$?

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