If 25.0 liters of neon at -25.0°C is allowed to expand to 55.0 liters, what must the new temperature be to maintain constant pressure?
i’m not sure
To solve this problem, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, let's convert -25.0°C to Kelvin. To do this, we use the formula:
T(K) = T(°C) + 273.15
So, -25.0°C + 273.15 = 248.15 K
We know the initial volume is 25.0 liters and the final volume is 55.0 liters. To maintain constant pressure, we can assume the number of moles and the gas constant will remain constant.
So we can rewrite the equation as:
P1V1 / T1 = P2V2 / T2
Solving for T2, we get:
T2 = (P2V2 * T1) / (P1V1)
Plugging in the given values, we have:
T2 = (P2 * 55.0 * 248.15) / (1 * 25.0)
Now, we need the value of P2, the final pressure. Since the question does not provide this information, we cannot determine the exact value of T2. To solve for T2, we would need the pressure at the final state.
Therefore, without knowing the pressure at the final state, we cannot determine the new temperature needed to maintain constant pressure.
(V1/T1) = (V2/T2)
Remember T must be converted to kelvin.
K = 273 + C