A sample of 4.59 L of CO2 gas has a pressure of 7.56 atm. What volume (in Liters) would the gas occupy if the pressure was reduced to 2.57 atm and the temperature raised from 25.0oC to 39.0oC?

The answer to your question is V = 14.44 L

Explanation:

Data

Conditions 1                            Conditions 2

V1 = 4.69 L                               V2 = ?

P1 = 7.56 atm                           P2 = 2.57 atm

T1 = 25°C                                  T2 = 39°C

Process

1.- Convert the temperature to °K

T1 = 25 + 273 = 298°K

T2 = 39 + 273 = 312 °K

2.- Find V2 using the combined gas law

     (P1V1)/T1 = (P2V2)/T2

solve for V2

     V2 = (P1V1T2) / (T1P2)

substitution

     V2 = (7.56 x 4.69 x 312) / (298 x 2.57)

Simplify

     V2 = 11062.39 / 765.86

Result

     V2 = 14.44 L

One example is when two glasses of water are being measured with the same temperature, but when you added another drop it doesn't change it's temperature. As you will notice each drop you add, the temperature doesn't add. But the heat contained in it is gradually getting higher each drop of water you add.

It is because heat and temperature is slight but significant, heat is the overall energy of the molecular motion, while temperature is the average energy of the molecular motion. Meaning to say Heat has a major part in the energy od the molecular motion.

Explanation:

I hope this one helped you :]