Question

If the temperature is held constant during this process and the final pressure is 671 torr , what is the volume of the bulb that was originally filled with gas

Answer 1

Complete Question

The  complete question is shown on the first uploaded image  

Answer:

Explanation:

From the question we are told that

   The initial pressure of the gas is  $P_1 = 1.50 \ atm$

   The volume of the second bulb is  $V_2 = 0.800 \ L$

   The  final pressure of the gas is  $P_2 = 671 \ torr = \frac{671 }{ 760} = 0.883 \ atm$

Let the unknown volume be represented as $V_1 = V \ L$

Generally from Boyle's law we have that

      $P_1 * V_1 = P_2 * V_2$

=>   $1.50 * V = 0.883 * 0.800$

=>   $V = 0.479 \ L$