Amylar balloon is filled with helium gas to a pressure of 107 kpa when the temperature is 22°c. if the temperature changes to 45°c, what will be the pressure of the helium in the balloon?

Explanation:

To solve this problem, we have to remember the ideal gas theory. We going to use the Gay Lussac Law.

The equation is:

PiTo = PoTi

Where:

Pi =initial pressure

Po = final pressure

Ti = initial temperature

To = final temperature

Let's use this equation and replace the values:

Pi = 107 kPa

Ti = 22°C

To = 45 °C

Po = ?

You can use the units as the problem gave you.

Using the Gay Lussac law:

107 kPa x 45 °C = Po x 22°C

Po = (4,815 kPa°C / 22°C) = 218.86 kPa

Po = 218 kPa

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e