The answer for the following problem is mentioned below.
- <u><em>Therefore the final volume of the gas is 52.7 ml.</em></u>
Explanation:
Given:
Initial pressure (
) = 290 kPa
Final pressure (
) = 104 kPa
Initial volume (
) = 18.9 ml
To find:
Final volume (
)
We know;
From the ideal gas equation;
P × V = n × R × T
where;
P represents the pressure of the gas
V represents the volume of gas
n represents the no of the moles
R represents the universal gas constant
T represents the temperature of the gas
So;
P × V = constant
P ∝ 
From the above equation;
represents the initial pressure of the gas
represents the final pressure of the gas
represents the initial volume of the gas
represents the final volume of the gas
Substituting the values of the above equation;
= 
= 52.7 ml
<u><em>Therefore the final volume of the gas is 52.7 ml.</em></u>
Answer:
It won't let me type this for some reason but here it is.
Answer:
112 L
Explanation:
Since the pressure is being held constant, you can use the following variation of the Ideal Gas Law to find the new volume:
In this equation, "V₁", "T₁", and "N₁" represent the initial volume, temperature, and moles. "V₂", "T₂", and "N₂" represent the final volume, temperature, and moles.
V₁ = 87.2 L V₂ = ? L
T₁ = 425 K T₂ = 273 K
N₁ = 2.5 moles N₂ = 2.5 + 2.5 = 5.0 moles
<----- Formula
<----- Insert values
<----- Simplify denominators
<----- Simplify left side
<----- Multiply both sides by 1365
To find the number of atoms in the sample of copper, we need its atomic mass and the use of the Avogadro's number to find the equivalent units in terms of atoms.
68.7 g Cu ( 1 mol / 63.55 g ) ( 6.022 x 10^23 atoms / 1 mol ) = 6.51 x 10^23 atoms Cu
