Answer:
V₂ = 568.9 mL
Explanation:
Given data:
Volume of gas = 550 mL
Pressure of a gas = 960 mmHg
Temperature = 200.0°C ( 200+273 = 473 K)
Final volume = ?
Final pressure = 830 mmHg
Final temperature = 150°C (150+273 = 423 K)
Solution:
Formula:
P₁V₁/T₁ = P₂V₂/T₂
P₁ = Initial pressure
V₁ = Initial volume
T₁ = Initial temperature
P₂ = Final pressure
V₂ = Final volume
T₂ = Final temperature
Solution:
V₂ = P₁V₁ T₂/ T₁ P₂
V₂ = 960 mmHg × 550 mL × 423 K / 473 K ×830 mmHg
V₂ = 223344000 mL / 392590
V₂ = 568.9 mL
The molar mass of the hydrate is 278.06
The molar mass of the anhydrous salt is 151.92
The molar mass of water in the hydrate is 126.14
B) there is an unequal number of electrons and protons
Answer:
(a) A strong acid
Explanation:
We have given the pH of the solution is 2.46
pH=2.46
So the concentration of 
solution having H+ concentration more than 
is acidic
Since in the given solution, H+ concentration is 0.00346 M which is more than 10^{-7}[/tex] so this is an acidic solution
Note-The concentration of 
decide the behavior of the solution that is, it is acidic or basic
Answer:
b.
Explanation:
. i got it from my smart friend
