The answer is the atomic mass.
Answer:
The number of moles of gas in the sample = 0.916 moles
Explanation:
Step 1: Data given
Volume of the container = 8.5 L
Temperature = 55 °C = 328 K
Pressure = 2.9 atm
Step 2: Calculate the number of moles of gas in the sample.
p*V = n*R*T
⇒with p = the pressure = 2.9 atm
⇒with V = the volume of the container = 8.5L
⇒with n = the number of moles of gas = ?
⇒with R = the gas constant = 0.08206 L*atm/mol*K
⇒with T = the temperature = 328 K
n = (p*V)/(R*T)
n = (2.9*8.5)/(0.08206*328)
n = 24.65 / 26.91568
n = 0.916 moles
The number of moles of gas in the sample = 0.916 moles
Are subatomic particles that are manifested by forces of attraction and repulsion between them through electromagnetisms
-good luck
Answer:
100 kPa
Explanation:
This can be solved with one of the gases law. This law establishes that the pressure of the gas is directly proportional to its temperature: If we increase the temperature, the pressure will increase.
In this case, we decrease the temperature, so its pressure will be lower.
P₁ / T₁ = P₂ / T₂
We convert T° to Absolutes Values
27°C + 273 = 300 K
-173°C + 273 = 100 K
300 kPa / 300 K = P₂ / 100 K
(300 kPa / 300 K) . 100K = P₂
P₂ = 100 kPa
This is the Charles Gay Lussac's law.
Answer:
The volume will be 82.67 L
Explanation:
Charles's Law is the relationship between the volume and temperature of a certain amount of ideal gas. In this way, Charles's law is a law that says that when the amount of gas and pressure are kept constant, the ratio between volume and temperature will always have the same value:
Having a certain volume of gas V1 that is at a temperature T1 at the beginning of the experiment, by varying the volume of gas to a new value V2, then the temperature will change to T2, and it will be true:
In this case, you know:
- V1= 40 L
- T1= 90 °C
- V2= ?
- T2= 186 °C
Replacing:
Solving:
V2= 82.67 L
<u><em>The volume will be 82.67 L</em></u>