### Problem: Lifting Scientific Equipment with Helium Balloons1. **Large helium-filled balloons are used to lift scientific equipment to high altitudes.** **(a)** What is the pressure inside such a balloon if it starts out at sea level with a temperature of 10 °C and rises to an altitude where its volume is twenty times the original volume and its temperature is −44 °C? $$ P_2 = \_\_\_\_\_\_\_\_ \text{ atm} $$ **(b)** What is the gauge pressure? (Assume atmospheric pressure is constant) $$ \text{Gauge pressure:} = \_\_\_\_\_\_\_\_ \text{ atm} $$### Explanation of Diagrams (if any)There are no graphs or diagrams presented in this problem statement. The exercise focuses on understanding the changes in pressure of a helium-filled balloon under specific conditions of temperature and volume change. ### Method for SolutionThis problem involves the use of the Ideal Gas Law and concepts related to pressure, volume, and temperature changes for gases. Specifically, one would likely need to use combined gas law relationships to solve for the unknown pressure after the conditions change.

Answered: Image /qna-images/answer/081f6cf0-1626-4b9b-ae44-5009a0b355ee.jpg

1. Large helium-filled balloons are used to lift scientific equipment to high altitudes. (a) What is the pressure inside such a balloon if it starts out at sea level with a temperature of 10 °C and rises to an altitude where its volume is twenty times the original volume and its temperature is -44 °C? P₂= atm (b) What is the gauge pressure? (Assume atmospheric pressure is constant.) Gauge pressure: atm

1. Large helium-filled balloons are used to lift scientific equipment to high altitudes. (a) What is the pressure inside such a balloon if it starts out at sea level with a temperature of 10 °C and rises to an altitude where its volume is twenty times the original volume and its temperature is -44 °C? P₂= atm (b) What is the gauge pressure? (Assume atmospheric pressure is constant.) Gauge pressure: atm