I need help with answering this question.
What is the absolute entropy of 1.9 mol of gaseous ammonia at 2.8 bar and 298 K?
To determine the absolute entropy of 1.9 mol of gaseous ammonia at 2.8 bar and 298 K, you need to use the equation:
ΔS = S_final - S_initial
First, you need to determine the initial entropy, S_initial. The initial entropy, in this case, will be taken as the entropy of ammonia at standard conditions (1 bar and 298 K), which can be found in tables or calculated using statistical thermodynamics.
Once you have the initial entropy, you can use the following equation to calculate the final entropy, S_final:
S_final = S_initial + R * ln (P_final / P_standard)
Where:
- S_initial is the initial entropy at standard conditions
- R is the gas constant (8.314 J/(mol*K))
- P_final is the final pressure (2.8 bar)
- P_standard is the standard pressure (1 bar)
Substituting the given values:
S_final = S_initial + R * ln (2.8 / 1)
Calculate the natural logarithm, ln(2.8 / 1), and multiply it by R. Then, add the result to the initial entropy to obtain the final entropy, S_final. This will give you the absolute entropy of 1.9 mol of gaseous ammonia at 2.8 bar and 298 K.