Question

how to solve
Combined gas law problem: A balloon is filled with 500.0 mL of He at a temperature of 72 ºC and 755 mm Hg. As the balloon rises in the atmosphere, the pressure and temperature drop. What volume will it have when it reaches an altitude where the temperature is -33 ºC and the pressure is 0.65 atm?


combined gas law: (P1V1)/T1 = (P2V2)/T2

760 mm Hg = 1.00 atm (exact)...

Answer 1

start by writing down everything that you have:
\(\sf P_1\) = 755 mmHg
\(\sf V_1\) = 500 mL
\(\sf T_1\) = 72.0 Celsius

\(\sf P_2\) = 0.65
\(\sf T_2\) = 33 celsius
\(\sf V_2\) = ?

Rearranging the forlmula to solve for \(\sf \color{red}{V_2}\). Think of algebra. Nothing more than a bit of tweeking to the formula to solve for the desired variable. Then, plug in and solve.

Answer 2

im lost