200 ml of a gas at 27oC and 1140 Pa pressure is transferred to a vessel of 450 ml capacity. What temperature is to be applied, if the pressure applied is 2000 Pa?

Dupl;icate post. See my other response

Use the Ideal Gas Law, and plug in the numbers. Remember that the temperature must be in Kelvins, so convert the 27 degrees celsius into kelvins, then plug in the numbers,

To solve this problem, we can use the ideal gas law, which states:

PV = nRT

Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature

In this case, we are given the initial volume (200 ml), initial temperature (27°C), and initial pressure (1140 Pa). We are also given the final volume (450 ml) and final pressure (2000 Pa). We can assume that the number of moles (n) of the gas remains constant.

First, we need to convert the initial temperature from Celsius to Kelvin, as the ideal gas law requires temperatures to be in Kelvin. To do this, we add 273.15 to the initial temperature:

Initial temperature in Kelvin = 27°C + 273.15 = 300.15 K

Now, let's calculate the initial number of moles (n) using the ideal gas law:

n = PV / RT

Substituting the known values:
n = (1140 Pa * 0.2 L) / (8.314 J/(mol·K) * 300.15 K)

Simplifying:
n = 0.0763 mol

Since the number of moles remains constant after the transfer, we can use the ideal gas law again to find the final temperature (Tf) required:

Tf = PV / nR

Substituting the known values:
Tf = (2000 Pa * 0.45 L) / (0.0763 mol * 8.314 J/(mol·K))

Simplifying:
Tf = 938.98 K

Therefore, the temperature that needs to be applied to the gas is approximately 938.98 K.