10.0 grams of a gas occupies 12.5 liters at a pressure of 42.0 mm Hg. What is the volume when the pressure has increased to 75.0 mm Hg? 6.72 L 7.00 L 22.3 L 0.143 L

 7.00 L

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

    (At constant temperature and number of moles)

where,

= initial pressure of gas  = 42.0 mm Hg

= final pressure of gas  = 75.0 mm Hg

= initial volume of gas   = 12.5 L

= final volume of gas  = ?

Therefore, the volume  when the pressure has increased to 75.0 mm Hg is 7.00 L

b) mutualism

hope this : )

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.