What temp would a fixed volume of gas need to be heated in order to double its pressure if it starts out at 25?
To determine the temperature at which a fixed volume of gas needs to be heated in order to double its pressure, we can use the ideal gas law.
The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
In this case, we have a fixed volume of gas (V), and we want to find the temperature (T) at which the pressure (P) doubles. Let's denote the initial pressure as P1 and the final pressure (when it doubles) as P2.
Using the ideal gas law, we have P1 * V = n * R * T1 (initial condition) and P2 * V = n * R * T2 (final condition).
Since we are assuming the number of moles (n) and the volume (V) remain constant, we can simplify these equations to P1 = R * T1 and P2 = R * T2.
Given that the initial pressure, P1, is 25, and we want to double it to achieve a final pressure, P2, we have P2 = 2 * P1.
Substituting these values into our simplified equations, we get 2 * R * T1 = R * T2.
Dividing both sides by R, we have 2 * T1 = T2.
Therefore, the temperature at which the fixed volume of gas needs to be heated in order to double its pressure is twice the initial temperature. If the initial temperature is 25°C, you need to heat the gas to 50°C (or 298 K to 573 K in Kelvin) to double its pressure.