What volume of water, in mL, is needed to dissolve 1.3×103 mg of carbon dioxide gas when the partial pressure of carbon dioxide above the water is 3.7 atm at 25 °C? The Henry's constant for carbon dioxide gas in water at 25 °C is 0.034 M/atm.

V = 0.2714 mL

Explanation:

Henry's Law:

∴ Kh CO2 = 0.034 M/atm The Henry's constant

∴ Partial pressure: P CO2 = 3.7 atm

⇒ C CO2 = P CO2 / Kh

⇒ C CO2 = 3.7 atm / 0.034 M/atm = 108.823 M (mol/L)

∴ molar mass CO2 = 44.01 g/mol

⇒ mol CO2 = (1.3 E3 mg)(g/1000 mg)(mol/44.01 g) = 0.03 mol CO2

volumen solution:

⇒ V sln = (0.03 mol)(L/108.823 mol) = 2.714 E-4 L

⇒ V sln = 0.2714 mL

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8

the answer is c i took the test