An ideal gas is kept in a 10-liter [L] container at a pressure of 2.5 atmospheres [atm] and a temperature of 310 kelvin [K]. If the gas is compressed until its pressure is raised to 5 atmospheres [atm] while holding the temperature constant, what is the new volume in units of liters [L]?

5 L.

Explanation:

From the question given above, the following data were obtained:

Initial volume (V1) = 10 L

Initial pressure (P1) = 2.5 atm

Final pressure (P2) = 5 atm

Final volume (V2) =.?

Since the temperature is constant, we shall apply the Boyle's law equation to determine the new volume of the gas. This can be obtained as follow:

P1V1 = P2V2

2.5 × 10 = 5 × V2

25 = 5 × V2

Divide both side by 5

V2 =25/5

V2 = 5 L

Thus, the new volume of the gas is 5 L

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

c. 4.54 x 10–12 j happens to be correct