A balloon contains helium gas expands from 230ml to 860 ml as more helium is added. What was the initial quantity of helium present if the expanded balloon contains 3.8x10^-4 mol, assuming constant temperature and pressure?

n₁ = 1.0× 10⁻⁴ mol

Explanation:

Given data:

Initial volume of balloon = 230 mL

Initial number of moles of He =?

Final number of moles of He = 3.8 × 10⁻⁴ mol

Final volume of balloon = 860 mL

Solution:

The given problem will be solve through Avogadro law,

"Number of moles of gas and volume are directly proportional to each other at constant temperature and constant pressure"

Mathematical relationship:

V₁/n₁ = V₂/n₂

No we will put the values.

230 mL  /n₁   = 860 mL/ 3.8 × 10⁻⁴ mol

n₁ = 230 mL× 3.8 × 10⁻⁴ mol/ 860 mL

n₁ = 874 × 10⁻⁴ mol. mL / 860 mL

n₁ = 1.0× 10⁻⁴ mol

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i