under a pressure of 1.0 atm , a confined gas has a volume of 750mL. at constant temperature, the pressure is increased until the
1 answer:
Answer:
1.23 atm
Explanation:
Given data
- Initial pressure (P₁): 1.0 atm
- Initial volume (V₁): 750 mL
- Final pressure (P₂): to be calculated
- Final volume (V₂): 610 mL
For a gas sample, <em>there is an inverse relationship between the pressure and the volume</em>, that is, when the pressure is increased, the volume decreases. Mathematically, for an ideal gas at constant temperature, we can find the final pressure using Boyle's law.
You might be interested in
Answer:
The boiling point of a 8.5 m solution of Mg3(PO4)2 in water is<u> 394.91 K.</u>
Explanation:
The formula for molal boiling Point elevation is :
= elevation in boiling Point
= Boiling point constant( ebullioscopic constant)
m = molality of the solution
<em>i =</em> Van't Hoff Factor
Van't Hoff Factor = It takes into accounts,The abnormal values of Temperature change due to association and dissociation .
In solution Mg3(PO4)2 dissociates as follow :
Total ions after dissociation in solution :
= 3 ions of Mg + 2 ions of phosphate
Total ions = 5
<em>i =</em> Van't Hoff Factor = 5
m = 8.5 m
= 0.512 °C/m
Insert the values and calculate temperature change:
Boiling point of pure water = 100°C = 273.15 +100 = 373.15 K
= 373.15 K[/tex]
21.76 = T - 373.15
T = 373.15 + 21.76
T =394.91 K