Question

15. A balloon has a volume of 1.2 liters at a pressure of 1.1 atm and a temperature of 25 °C. If thetemperature changes to 75 °C and the volume changes to 6.7 liters, what is the new pressure?

Answer 1

The final pressure of the gas inside the ballon is 0.17 atm.

To solve this problem, we would need to use ideal gas equation.

Combined Gas Equation

This is a combination of the three major gas laws which are Boyle's law, Charles law and Pressure Law.

This is given as

`(p_1v_1)/(t_1)=(p_2v_2)/(t_2)`

we can define our variables

V1 = 1.2L

P1 = 1.1 atm

T1 = 25°C = (25 + 273.15)K = 298.15K

V2 = 6.7L

T2 = 75°C = (75 + 273.15)K = 348.15K

P2 = ?

Let's substitute the values into the equation above and solve for the final pressure

`\begin{gathered} (p_1v_1)/(t_1)=(p_2v_2)/(t_2) \\ p_2=(p_1v_1t_2)/(v_2t_1) \\ p_2=(1.1*1.2*348.15)/(6.7*298.15) \\ p_2=0.17\text{atm} \end{gathered}`

The final pressure of the gas inside the ballon is 0.17 atm.