29. A gas has a volume of 1.75 L at -23°C and 150.0 kPa.
At what temperature would the gas occupy 1.30 L at
210.0 kPa?

The answer for the following mention bellow.

Explanation:

Given:

Initial pressure () = 150.0 kPa

Final pressure () = 210.0 kPa

Initial volume () = 1.75 L

Final volume () = 1.30 L

Initial temperature () = -23°C = 250 k

To find:

Final temperature ()

We know;

According to the ideal gas equation;

P × V = n × R ×T

where;

P represents the pressure of the gas

V represents the volume of the gas

n represents the no of moles of the gas

R represents the universal gas  constant

T represents the temperature of the gas

We know;

= constant

× =

Where;

() represents the initial pressure of the gas

() represents the final pressure of the gas

() represents the initial volume of the gas

() represents the final volume of the gas

() represents the initial temperature of the gas

() represents the final temperature of the gas

So;

=

() =260 k

Therefore the final temperature of the gas is 260 k

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.

im pretty sure its b