Consider 3 liters of an ideal (monatomic) gas at a pressure of 34 atm and a temperature of 356K. Call this state of the system A. Using the ideal gas law, calculate the number of moles of gas present in the system.
3.49
The temperature of the system is reduced, keeping the volume constant at 3 liters, until the pressure of the gas in the system equals 13 atm. Call this new state of the system B. Calculate the temperature at this new state B in degrees K.
1.36×102
Now allow the gas to expand at constant pressure (13 atm) until the temperature is again equal to 356K. Call this state of the system C. Calculate the volume of the gas at state C. Enter your answer as a volume in liters.
7.85
Now calculate the work done on or by the system when the system moves back from state C to state A along the path CBA. Enter your answer in joules with the correct sign.
Calculate the heat absorbed or liberated by the system when the system moves from state C to state B. Enter your answer in joules with the correct sign.
Using your results from the previous two questions, calculate the heat absorbed or liberated by the system as the system moves from state B to state A. Enter your answer in joules with the correct sign.
It is possible to move from state C to state A in two stages via an alternative state D. The first step, from state C to state D involves increasing the pressure at constant volume until the pressure equals the original 34 atm. Calculate the temperature at the state D in degrees K.
Calculate the heat released or absorbed by the system as the system moves from state C to state D. Enter your answer in joules with the correct sign.
Calculate the work done on or by the system as it changes from state D to state A -- a change in volume at a constant pressure of 34 atm. Enter your answer in joules with the correct sign.
Use your answers to the previous two questions to calculate the heat change when the system moves from state D to state A. Enter your answer in joules with the correct sign.
if you just give me the formulas I should be able to figure it out. Please help me
1. pV =νRT
34 atm = 3445050 Pa
ν = pVRT = 3445050• 3•10^-3/8.31•356 = 3.49 mol
2.
V1=V2
p1 /T1 = p2 /T2
T2 =p2•T1/p1 =13•356/34 = 136 K
3. V1/T1 = V2/T2
V2 = V1•T2/T1 =3•356/ 136= 7.85 L
Sure! I can explain the formulas and steps to calculate the various quantities.
1. To calculate the number of moles of gas present in the system at state A, you can use the ideal gas law equation:
PV = nRT
Where,
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/(mol.K))
T = temperature (in Kelvin)
Rearranging the equation, n = PV / RT, substitute the given values to find the number of moles.
2. For the second part, to calculate the temperature at state B, you need to use Charles's Law, which states that at constant pressure, the volume of a gas is directly proportional to its temperature. So the ratio of initial and final temperatures is equal to the ratio of initial and final volumes.
T1 / T2 = V1 / V2
Rearranging the equation, T2 = T1 * (V2 / V1), substitute the given values to find the temperature at state B.
3. To calculate the volume at state C, you can use the combined gas law equation, which relates the initial and final states of the gas when pressure and temperature change, but the number of moles is constant. The equation is:
P1 * V1 / T1 = P2 * V2 / T2
Rearranging the equation, V2 = (P1 * V1 * T2) / (P2 * T1), substitute the given values to find the volume at state C.
4. The work done on or by the system when the system moves back from state C to state A along the path CBA can be calculated using the formula:
Work = P * (Vfinal - Vinitial), where P is the constant pressure and Vfinal and Vinitial are the final and initial volumes, respectively.
5. The heat absorbed or liberated by the system when the system moves from state C to state B can be calculated using the formula:
Heat = n * R * (Tfinal - Tinitial), where n is the number of moles, R is the ideal gas constant, and Tfinal and Tinitial are the final and initial temperatures, respectively. Note that if heat is absorbed, the value will be positive, and if heat is released, the value will be negative.
6. The heat absorbed or liberated by the system as it moves from state B to state A can be calculated using the same formula as above, but with the appropriate final and initial temperatures.
7. To calculate the temperature at state D, you can use the same formula as in step two, using the given pressures and the constant volume.
8. The heat released or absorbed by the system as it moves from state C to state D can be calculated using the same formula as in step five, but with the appropriate final and initial temperatures.
9. The work done on or by the system as it changes from state D to state A (a change in volume at a constant pressure of 34 atm) can be calculated using the same formula as in step four, with the appropriate final and initial volumes.
10. Finally, you can use the heats calculated in step eight and the work calculated in step nine to calculate the heat change when the system moves from state D to state A using the equation:
Heat = Heat_D_to_A - Work_D_to_A, where Heat_D_to_A is the heat released or absorbed by the system when it moves from state C to state D, and Work_D_to_A is the work done on or by the system as it changes from state D to state A.
I hope this explanation helps! Let me know if you have any further questions.