Calculating Final Temperature of Hydrogen Gas

[J_B__]

I need a little help getting this one started...

1.5 kg of Hydrogen gas at 8 bars and 27 degrees C are contained in a constant pressure piston-cylinder arrangement. Heat in the amount of 1740 kJ is added to the Hydrogen from a reservior at 400 degrees K. Determine: the final temperature of the Hydrogen Gas, the entropy change in the Hydrogen gas in kJ/degree K, the entropy change of the overall process (system and surroundings) in kJ/degree K, is the process reversible, irreversible, possible, or impossible?

(I think i can get the last three parts, but i cannot seem to figure out how to get the final temperature)

Thanks

 

[Navin A S]

!The final temperature of the Hydrogen gas can be calculated using the ideal gas law. The equation is 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 this case, we know the pressure (8 bars), the volume (1.5 kg of Hydrogen), and the number of moles (n=1.5/2.01588). Rearranging the equation to solve for T, we get T = PV/(nR). Plugging in the values given, we get T = 8*1.5/[(1.5/2.01588)*8.314] = 393.1 K. Therefore, the final temperature of the Hydrogen gas is 393.1 K.

 

[ravenprp]

for reaching out for help with this problem! Calculating the final temperature of the hydrogen gas may seem daunting, but let's break it down step by step. First, we need to determine the initial state of the hydrogen gas. We know that it has a mass of 1.5 kg, a pressure of 8 bars, and a temperature of 27 degrees C. We can use the ideal gas law to calculate the initial volume of the hydrogen gas.

PV = nRT

Where P is pressure, V is volume, n is number of moles, R is the ideal gas constant (8.314 J/mol*K), and T is temperature.

We can rearrange this equation to solve for volume:

V = nRT/P

Since we know the mass of the hydrogen gas (1.5 kg) and its molar mass (2.016 g/mol), we can calculate the number of moles present:

n = m/M = (1.5 kg)/(2.016 g/mol) = 0.744 mol

Now we can plug in all of our values to solve for the initial volume:

V = (0.744 mol)(8.314 J/mol*K)(300 K)/(8 bar) = 232.9 L

Next, we need to use the first law of thermodynamics to calculate the final temperature of the hydrogen gas. The first law of thermodynamics states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system:

ΔU = Q - W

In this case, we are given the amount of heat added to the hydrogen gas (1740 kJ) and we know that the process is taking place at constant pressure, so the work done by the system is simply the pressure multiplied by the change in volume:

W = PΔV

We can calculate the change in volume by using the ideal gas law again, but this time we are solving for the change in volume:

ΔV = nRΔT/P

Since the initial and final pressures are the same, we can cancel them out:

W = PΔV = P(nRΔT/P) = nRΔT

Now we can plug in all of our values to solve for the change in internal energy:

ΔU = Q - W = 1740 kJ - (0.744 mol)(8.314 J/mol*K)(