Respuesta :
Answer:
- The pressure of a gas increases four times, when the absolute temperature is increased four times, while maintaining the volume constant.
Explanation:
The expression that rules the change of temperature of ideal gases at constant volume is the Law of Gay-Lussac: pressure and temperature of gases are directly related. In the form of equations that is:
- P / T = constant
- P₁ / T₁ = P₂ / T₂ .......... [equation 1]
The question states that the absolute temperature is increased four times, the you can write that as T₂ = 4 × T₁, and substitute in the equation 1 to obtain:
- P₁ / T₁ = P₂ / (4 × T₁)
Simplify:
- P₂ = P₁ × 4 × T₁ / T₁ = P₁ × 4
That proves that the pressure also increases four times, when the absolute temperature is increased four times, while maintaining the volume constant.
Answer: The pressure will also increase 4 times.
Explanation:
To calculate the final temperature of the system, we use the equation given by Gay-Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.
Mathematically,
[tex]\frac{P_1}{T_1}=\frac{P_2}{T_2}[/tex]
where,
[tex]P_1\text{ and }T_1[/tex] are the initial pressure and temperature of the gas.
[tex]P_2\text{ and }T_2[/tex] are the final pressure and temperature of the gas.
We are given:
[tex]P_1=p\\T_1=t\\P_2=?=\\T_2=4t[/tex]
Putting values in above equation, we get:
[tex]\frac{p}{t}=\frac{P_2}{4t}\\\\P_2=4p[/tex]
Hence, the pressure will also increase 4 times.
