no.2 -A/kTno.1QUESTION 8Consider the reaction described in the previous problems.Use the following expression,no.1e-4/2kTto calculate the ratio of H atoms to H2 molecules in a hydrogen gas in thermal equilibrium with a reservoir at 1,094 K when thereare 6 x 1040 molecules m of H2.Recall that A = 4 eV and that a convenient approximation for the quantum density is given byno-(1030 m-)(m/m/2(T/300 K)/2,where the value of the temperature in K must be inserted for T, and the ratio of m/m, is the atomic mass (in atomic mass units,amu) for an atom, or the sum of atomic masses (in amu) for atoms in a molecule.Write the numerical answer in exponential form accurate to 2 decimal places, as described in the worksheet instructions(X.XXE+Y or X XXE-Y).Click Save and Submit to save and submit. Click Save All Answers to save all answers.Type here to search

Answered: Image /qna-images/answer/0c172230-ae5a-4338-9ad8-fd984d70fb3a.jpg

QUESTION 8 Consider the reaction described in the previous problems. Use the following expression, no.1 n2 no.2 n2 e-4/2kT to calculate the ratio of H atoms to H2 molecules in a hydrogen gas in thermal equilibrium witha reservoir at 1,094 K when there are 6 x 1020 molecules m3 of H2- Recall that A = 4 eV and that a convenient approximation for the quantum density is given by no =(1030 m-)(m/m3/2(T/300 K)3/2, where the value of the temperature in K must be inserted for T, and the ratio of m/m, is the atomic mass (in atomic mass units, amu) for an atom, or the sum of atomic masses (in amu) for atoms in a molecule. Write the numerical answer in exponential form accurate to 2 decimal places, as described in the worksheet instructions (X.XXE+Y or X. XXE-Y).

QUESTION 8 Consider the reaction described in the previous problems. Use the following expression, no.1 n2 no.2 n2 e-4/2kT to calculate the ratio of H atoms to H2 molecules in a hydrogen gas in thermal equilibrium witha reservoir at 1,094 K when there are 6 x 1020 molecules m3 of H2- Recall that A = 4 eV and that a convenient approximation for the quantum density is given by no =(1030 m-)(m/m3/2(T/300 K)3/2, where the value of the temperature in K must be inserted for T, and the ratio of m/m, is the atomic mass (in atomic mass units, amu) for an atom, or the sum of atomic masses (in amu) for atoms in a molecule. Write the numerical answer in exponential form accurate to 2 decimal places, as described in the worksheet instructions (X.XXE+Y or X. XXE-Y).

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter3: The Second And Third Laws Of Thermodynamics

Section: Chapter Questions

Problem 3.7E

See similar textbooks

Similar questions

The equilibrium pressure of H2 over U(s) and UH3(s) between 450 K and 715 K fits theexpression ln (p/Pa) = A + B/T + C ln(T/K), with A = 69.32, B = - 1.464 x 104 K, and C = -5.65. Find an expression for the standard enthalpy of formation of UH3(s) and from itcalculate fC°p.
2. Find ??sys, ??surr, q, w, and ?? for the reversible isothermal expansion of 3.000 mol of argon (assumed ideal) from a volume of 100.0 L to a volume of 500.0 L at 298.15 K.
A sample of K(s) of mass 3.226 gg undergoes combustion in a constant volume calorimeter at 298.15 K. The calorimeter constant is 1849 J⋅K−Mol-, and the measured temperature rise in the inner water bath containing 1538 gg of water is 1.776 K. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1CP,m(H2O,l)=75.3J⋅mol−1⋅K−1. 1) Calculate ΔU��f for K2O 2) Calculate ΔH∘f for K2O
Suppose that the gas-phase reaction 2 NO1g2 + O21g2 ¡2 NO21g2 were carried out in a constant-volume containerat constant temperature. (a) Would the measured heatchange represent ΔH or ΔE? (b) If there is a difference, whichquantity is larger for this reaction? (c) Explain your answer topart (b).
1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.
A 5.00 dm3 gas cylinder containing 4.00 kg of NH3(g) at 27oC developed a leak leading to the escape of the gas into the atmosphere. If the atmospheric pressure is 101.3 kPa, calculate the PV work done by the gaas, assuming ideal behavior.
The conversion of oxygen into ozone in the upper atmosphere is as follow : 3232 O2(g) → O3(g), with ΔH298 = +143kJ at 298K. Cp(O2) = 29.355 J/Kmol; Cp(O3) = 39.2 J/K The enthalpy of formation at 200K is : a. ΔH200 = -143 473J b. ΔH200 = -142 527J c. ΔH200 = +142 527J d. ΔH200 = +143 473J
ammonia (considered to be an ideal gas) initially at 25 C and 1 bar pressure is heated at constant pressure until the volume tripled. Calculate the q per mole, w per mole, delta H, delta U, and delta S, given that CP=25.895 + 32.999 x 10-3 T – 30.46 x 10-7 (T)2 ? (J/K mol)
Find the internal energy of 30 g of Argon gas (Ar) at 90°C. (Molar mass of Argon; Mr = 40 g mol-1, Avogadro constant; NA = 6.022 ×1023 mol-1, Boltzmann constant; k = 1.38 ×10-23 JK-1)
AuBr(s) + 2 CN– (aq) ⇄ [Au(CN)2]– (aq) + Br– (aq) Given: Keq = 2.02 x 1033 Ksp for AuBr is 9.8 x 10–6, Solve for the Kf of [Au(CN)2]–
If 4.00 moles of hydrogen (C p = 28.8 J mol-1 K -1 ) are expanded reversibly andisothermally at 400K from an initial volume of 12.0L to a final volume of 30.0L,calculate DE, q, w, DH, and DS for the gas. Assume ideal gas behavior.
A quantity of 0.277 moles of an ideally behaving gas expands isothermally and reversibly from a volume of 5L to twice that volume at 27 ° C. What will be the value of Q, W, ΔU, and ΔH?