The Henry's Law constant (k) for carbon monoxide in water at 25°C is 9.71 x 10-4 mol/(L·atm). How many grams of CO will dissolve in 1.00 L of water if the partial pressure of CO is 2.75 atm? A) 3.53 x 10-4 g D) 7.48 x 10-2 g B) 2.67 x10-3 g E) None of these choices is correct. C) 9.89 x 10-3 g

2.67 * 10-3 mol/L

Explanation:

Henry's law is a gas law that states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid. The proportionality factor is called Henry's law constant. (Wikipedia)

Given that; C =kP

C=concentration of a dissolved gas = ?

k=Henry's Law constant = 9.71 x 10-4 mol/(L·atm)

P=partial pressure of the gas = 2.75 atm

So,

C = 9.71 x 10-4 mol/(L·atm) * 2.75 atm

C = 2.67 * 10-3 mol/L

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

lol idk man i guess u gotta ask bill nye the science guy