Calculate A, E, μ, cv and S for 1 mole of Kr at 298 K and 1 atm (assuming ideal behavior) Calculate A, E, μ, cv and S for 1 mole of Kr at 298 K and 1 atm (assuming ideal behavior)
Calculate the entropy of a mixture of 50% Ne and 50% Ar at 500 K and 10 atm, assuming ideal behavior. Calculate the entropy of a mixture of 50% Ne and 50% Ar at 500 K and 10 atm, assuming ideal behavior.
1. a 10 mol sample of ideal gas whose heat capacities are Cv= 20.8 J/K Mole and Cv = 29.1 J/K Mole a. Undergoes a reversible constant volume cooking from 49.3 L, 300 K, and 5.00 atm to 150 K. Calculate q, w, and ΔU. b. the same gas then underwent a reversible constant pressure expansion from 150 K and 2.50 atm to 98.6 L. Calculate q , w, and ΔU. You'll need the ideal gas law to calculate T-final...
1. Compute the following quantities for a system with 1.0 mol of Kr at 298 K and 1.0 atm. For this problem, assume that Kr is ideal gas (indistinguishable particles) and electronic contribution to the partition function can be ignored. For part (b)-(d). clearly indicate how each quantitiy is related to the partition function, Q. (a) Single-particle partition function, q. (b) Helmholtz free energy, A. (c) Average energy of the system, (E). (d) Entropy, S. (e) Constant volume heat capacity,...
3 pts Question 4 ay с Calculate the pressure (atm) of 1 mole of hydrogen gas at 298 K using the Van der Waals equation for a gas in a 30.0 L flask 3 pts Question 5 Calculate the pressure (atm) of 1 mole of hydrogen gas at 298 K using the Van der Waals equation for a gas in a 1.00 L flask 3 pts Question 6 Calculate the pressure (atm) of 1 mole of hydrogen gas at 298...
One mole of a monatomic perfect gas, initially at 298 K and 1 atm, expands irreversibly and isothermally against 0.5 atm, doing 400 J of work in the process. Calculate or explain the values of DU, DH, DG, q, DSsys, DSsurr and DStot. Also, calculate the reversible work for this isothermal change of state.
The observed pressure of a 2.963-mole sample of Kr(g) in a 9.450-L container is 1.782 atm. Use the van der Waals equation to determine the pressure if the gas were behaving ideally. Kr(s) = 2.32 atm. L2 mol Our(s) = Ideal pressure atm
1. 50 ce/s of O2 at 1 atm is heated from 298 to 3000 K. Calculate the rate of heat transfer. Be sure to account for dissociation 1. 50 ce/s of O2 at 1 atm is heated from 298 to 3000 K. Calculate the rate of heat transfer. Be sure to account for dissociation
A 0.825 mol sample of NO2(g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 19.3 K. Assuming ideal gas behavior, calculate the amount of heat (?) in joules required to affect this temperature change and the total change in internal energy, Δ?. Note that some books use Δ? as the symbol for internal energy instead of Δ?.
A 0.825 mol sample of NO2(g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 19.3 K. Assuming ideal gas behavior, calculate the amount of heat (?) in joules required to affect this temperature change and the total change in internal energy, Δ?. Note that some books use Δ? as the symbol for internal energy instead of Δ?.
1. State whether the behavior of methylamine (CH,NH2) would be less ideal than that of argon. 2. Calculate the value of R in L-atm/mol-K by assuming that an ideal gas occupies 224 L/mol at STP Why do you equalize the water levels in the bottle and the beaker? 3. Why does the vapor pressure of water contribute to the total pressure in the bottle? 4. What is the value of an error analysis? 5. 6. Suggest reasons why real gases...