A sample container of carbon monoxide occupies a volume of 435 ml at a pressure of 785 torr and a temperature of 298 k. What would its temperature be if the volume were changed to 265 ml at a pressure of 785 torr?

If the volume of the carbon monoxide was to change to the given volume, the temperature will also change to 181.5 Kelvins.

Given the data in the question;

Initial Temperature;

To determine the final temperature, we use the Equation from Charles's Law:

We substitute our given values into the equation;

Therefore, if the volume of the carbon monoxide was to change to the given volume, the temperature will also change to 181.5 Kelvins.

Learn more: link

181.54 K

Explanation:

From gas laws, we know that v1/t1= v2/t2 where v and t represent volume and temperatures, 1 and 2 for the first and second container. Making t2 the subject of the formula then

T2=v2t1/ v1

Given information

V1 435 ml

V2 265 ml

T1 298K

Substituting the given values then

T2=265*298/435=181.54 K

1= 26.17

2= 1.17

3=30.86

4=5.86

just took the assigment on edge