a gas is contained in a thick - walled balloon under the conditions 777 torr, 495 k, and 1.53 l. the volume…

Explanation:

Step1: Convert initial pressure to atm

1 atm = 760 torr, so $P_1 = 777\ torr\times\frac{1\ atm}{760\ torr}\approx1.022\ atm$

Step2: Apply combined - gas law formula

The combined - gas law is $\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$. We want to find $P_2$. Rearranging the formula gives $P_2=\frac{P_1V_1T_2}{V_2T_1}$. Substitute $P_1 = 1.022\ atm$, $V_1 = 1.53\ L$, $T_1 = 495\ K$, $V_2 = 2.58\ L$, and $T_2 = 368\ K$ into the formula. $P_2=\frac{1.022\times1.53\times368}{2.58\times495}$

Step3: Calculate the value of $P_2$

$P_2=\frac{1.022\times1.53\times368}{2.58\times495}=\frac{1.022\times569.36}{1277.1}=\frac{581.886}{1277.1}\approx0.456\ atm$ Convert back to torr: $P_2 = 0.456\ atm\times760\ torr/atm = 346.56\ torr\approx347\ torr$

Answer:

347 torr