A6.0 l container holds a sample of hydrogen gas at 150 kpa. if the pressure increases to 2 atm and the temperature remains constant, what will the volume be?

The volume will be 4.44 L

Explanation:

Data:

First volume, V1 = 6 L

First pressure, P1 = 150 kPa -> 150 kPa * 1 atm/101.325 kPa = 1.48 atm

Second pressure, P2 = 2 atm

Second volume, V2 = ? L

From Boyle's law:

P1*V1 =P2*V2

V2 = P1*V1/P2

V2 = 1.48*6/2

V2 = 4.44 L

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.