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

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."

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