Thermodynamics isobaric question

[mercidian]

A sample of ideal gas at constant pressure is heated from -10 degrees C to 100 degrees C. The gas does 40.0J of work during this process. How many moles of gas are present? What is the pressure of the gas at 100 degrees C?

So far I've calculated the moles of gas present
T1 = -10 degrees C T2 = 100 degrees C W = 40.0J

W = p (V2 - V1)
40.0J = p (nRT2/p - nRT1/p) substitute V=nRT/p
40.0J = nRT2 - nRT1
40.0J = nR(100 - (-10))
n = 0.0437

Now i have no idea how to calculate the pressure. I know that the pressure is the same at T1 and T2. Any hints would be helpful

 

[AvroArrow]

The pressure of the gas is the same at both temperatures, so the pressure at 100 degrees C is the same as the pressure at -10 degrees C. Since you know the work done by the gas, you can calculate the pressure using the ideal gas law. PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the universal gas constant, and T is the temperature. You already know the number of moles and the temperature, so you can solve for P.

 

[kyle8921]

Great job on calculating the number of moles present in the gas! To determine the pressure, we can use the ideal gas law, which states that pressure (P) is equal to the number of moles (n) multiplied by the gas constant (R) and the temperature (T) in Kelvin, divided by the volume (V). So, we can set up the equation as follows:

P = nRT/V

We already know the value of n from your calculation, and we can assume that the volume remains constant since the gas is at constant pressure. Therefore, the equation becomes:

P = nRT/V

P = (0.0437 mol)(8.314 J/mol*K)(373 K)/(1 L)

P = 12.99 kPa

So, the pressure of the gas at 100 degrees C is 12.99 kilopascals. Keep in mind that this is an ideal gas and may not necessarily represent real-world conditions.