Answer:
P₂ = 592.7 torr
Explanation:
Given data:
Initial Pressure = 215 torr
Initial volume = 51.0 mL
Final pressure = ?
Final volume = 18.5 mL
Solution:
P₁V₁ = P₂V₂
P₁ = Initial Pressure
V₁ = Initial volume
P₂ = Final pressure
V₂ = Final volume
Now we will put the values in formula.
P₁V₁ = P₂V₂
215 torr × 51.0 mL = P₂ × 18.5 mL
10965 mL. torr = P₂ × 18.5 mL
P₂ = 10965 mL. torr /18.5 mL
P₂ = 592.7 torr
Both have "Pendent" in the word.
Answer:
In the gas there are 6.02x10²² molecules
Explanation:
This is a problem to be solved by the Ideal Gas Law formula, which is this one:
Pressure . volume = n° moles . R . T° in K
The excersise presented R as 8.31 J/mol, but If i follow the others data, I'd rather use 0.082 L.atm / mol.K
Let's replace numbers:
2.5 atm . 1L = n° moles. 0.082L.atm / mol.K . 303K
(2.5 atm . 1L) / (0.082 mol.K/L.atm . 303K) = n° moles
0.100 moles = n
Now that we have the moles, we can use NA to calculate the total of molecules:
1 mol ___ has __ NA molecules
0.1 mol has ____ ( 0.1 . 6.02x10²³) = 6.02x10²² molecules
Aluminum because it’s a conductor, glass is more so of an insulator.