A sample of gas occupies 100.0 mL at standard pressure. What volume will the gas occupy at a pressure of 80.0 mm Hg if the temperature remains constant? *

950mL

Explanation:

The following were Data were obtained from the question:

Initial volume (V1) = 100mL

Initial pressure (P1) = stp = 760mmHg

Final pressure (P2) = 80mmHg

Final volume (V2) =..?

The final volume of the gas can be obtained by using the Boyle's law equation as follow:

P1V1 = P2V2

760 x 100 = 80 x V2

Divide both side by 80

V2 = (760 x 100) /80

V2 = 950mL

Therefore, the new volume of the gas is 950mL

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.