If 15.0 liters of neon at 25.0 °C is allowed to expand to 45.0 liters, what must the new temperature be to maintain constant pressure?
Question
If 15.0 liters of neon at 25.0 °C is allowed to expand to 45.0 liters, what must the new temperature be to maintain constant pressure?
Solution
To solve this problem, we can use the ideal gas law equation, which states that the product of the volume and temperature of a gas is constant if the pressure and amount of gas are constant. This can be written as:
V1/T1 = V2/T2
where: V1 = initial volume = 15.0 liters T1 = initial temperature = 25.0 °C = 298.15 K (converted from Celsius to Kelvin by adding 273.15) V2 = final volume = 45.0 liters T2 = final temperature = ?
We can rearrange the equation to solve for T2:
T2 = V2 * T1 / V1
Substituting the given values:
T2 = 45.0 liters * 298.15 K / 15.0 liters
T2 = 894.45 K
So, the new temperature must be 894.45 K to maintain constant pressure.
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