Question

Consider the 0.5 mol sublimation of solid A described below: A (solid, 1 bar, 750 K)...

Consider the 0.5 mol sublimation of solid A described below: A (solid, 1 bar, 750 K) ⇄ A (gas, 1 bar, 750 K) Since the sublimation enthalpy of A is 481.2 J / mol, determine ΔU (in J). *
1/1
-2877
0.96
-9353

procedure please

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Q1: The entropy of sublimation of a certain compound is 5.2 J K–1 mol–1 at its...
Q1: The entropy of sublimation of a certain compound is 5.2 J K–1 mol–1 at its normal sublimation point of 72 °C. Calculate the vapour pressure (in torr) of the compound at 33 °C. Assume that the enthalpy of sublimation is constant. I get 1586.851385 torr Q2: Compound       So (J K–1 mol–1) A 20 B 96 C 74 D 36 At 298 K, ΔGo is 129 kJ / mol for the reaction 3A + 2B == 2C + 2D Calculate...
Calculate deltaS for N2 (1 bar, 298 K) --> N2 (32 bar, 1500 K). Assume N2...
Calculate deltaS for N2 (1 bar, 298 K) --> N2 (32 bar, 1500 K). Assume N2 to be an ideal gas. CP = 28.58 + 3.77 x 10-3 T – 0.50 x 105 T-2 J K-1 mol-1
A mixture of 85% n-heptane, remaining cyclohexane gas at 1 bar and 308 K is compressed...
A mixture of 85% n-heptane, remaining cyclohexane gas at 1 bar and 308 K is compressed to a final state at 1443.47 K and 64.475 bar. Estimate the enthalpy and entropy changes for the process using residual properties and by the Lee/Kessler correlations. In its initial state, the system may be assumed an ideal gas. please answer asap
4. In a gaseous sample containing 4 mol of ClF at T K and 1 bar,...
4. In a gaseous sample containing 4 mol of ClF at T K and 1 bar, how many moles of molecules are in the first excited vibrational state? Treat the gas as non-interacting with Θvib = 1132 K.
A sample containing 2.50 moles of He (1 bar, 345 K ) is mixed with 1.75...
A sample containing 2.50 moles of He (1 bar, 345 K ) is mixed with 1.75 mol of Ne (1 bar, 345 K ) and 1.50 mol of Ar (1 bar, 345 K ). Calculate ΔGmixing. Calculate ΔSmixing. Express your answer with the appropriate units. Calculate ΔA for the isothermal compression of 3.11 mol of an ideal gas at 321 K from an initial volume of 60.0 L to a final volume of 20.5 L.​ Does it matter whether the...
In a gaseous sample containing 4 mol of ClF at 514 K and 1 bar, how...
In a gaseous sample containing 4 mol of ClF at 514 K and 1 bar, how many moles of molecules are in the first excited vibrational state? Treat the gas as non-interacting with capital theta subscript v i b end subscript = 1132 K.
Consider the solid S described below. The base of S is the region enclosed by the...
Consider the solid S described below. The base of S is the region enclosed by the parabola y = 1 - 9x^2 and the x-axis. Cross-sections perpendicular to the x-axis are isosceles triangles with height equal to the base. Find the volume V of this solid.
2.15 mol of an ideal gas with CV,m=3R/2 undergoes the transformations described in the following list...
2.15 mol of an ideal gas with CV,m=3R/2 undergoes the transformations described in the following list from an initial state described by T=350.K and P=5.00bar. 1) The gas undergoes a reversible adiabatic expansion until the final pressure is one-fourth its initial value. 2) The gas undergoes an adiabatic expansion against a constant external pressure of 1.25 bar until the final pressure is one-fourth its initial value. 3)The gas undergoes an expansion against a constant external pressure of zero bar until...
Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute the molar delta...
Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute the molar delta H (in kJ/mol) for this reaction at 298 K and a pressure of 30 bar. Joule-Thomson coefficients and heat capacities are listed in the table below: Compound Cp (cal mol^-1 K^-1) Joule-thomson coefficient (K/bar) CO 6.3423 + 0.0018363 T 1.20 O2 6.148 + 0.003102 T 1.15 CO2 6.369 + 0.0101 T 1.10
Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute the molar delta...
Consider the reaction CO (g) + 0.5 O2 (g) -> CO2 (g). Compute the molar delta H (in kJ/mol) for this reaction at 298 K and a pressure of 30 bar. Joule-Thomson coefficients and heat capacities are listed in the table below: Compound Cp (cal mol^-1 K^-1) Joule-thomson coefficient (K/bar) CO 6.3423 + 0.0018363 T 1.20 O2 6.148 + 0.003102 T 1.15 CO2 6.369 + 0.0101 T 1.10