The constantheat capacity ofperpectwith temperature according to the expressionaa cample ofZAMOOTMAprers urefren of punad SOMpoundCP / (J K-')gas2 20.170.34 68 CT7K). calculare qi Wi AU and AH whentemperature iš raised promto 100 °C, Ci) at constantol sig oldenieoh oe25°0pressure,(i)dt constant voume.

The above problem is thermodynamic problem. At constant pressure and at constant volume , Perfect…

Answered: The constant heat capacity oe a sample…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 1ALQ

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1 what's between.. Hhe differerce 2) Arasume the gas rticles within this contairer behoves ike finod Intial T=100k T= 200K farwing relactionships cen in final of the be used nd al to statep ?, Expuin why!! %3D
Which one of the following is TRUE about AH°ffor the substances given? a. AH°ffor Br2(e) = 0 O b. AH°; for He(e) = 0 O c. AH°ffor N2(e) > O O d. AH°ffor O(g) < 0 O e. None of these is true
Given R= 8.31 J mol·' K-' mol', k= 1.38 x10-23 J K-', NA = 6.23 x 10²3 mol- 1. Calculate a) the mean translational kinetic energy of carbon dioxide molecule with a relative molecular mass of 44 at 20 °C [ans: 6.07×10-21 J] b) the mean translational kinetic energy of a molecule on an ideal gas at 10 °C? [ans: 5.86×10-21 J]
1. PCl (9)2 PCl, (9) +C1, (g) a 500 kelvin kp 0.497 %3D in an equulibrium miXTLIYe at 500 K, = 0.800 atm and Ppet =0.350 atm. What w PEn in he equiliorium mixtire
CH3 Quis I Argon o an ideal gas. Finicd the charge mo lar entra py when the gas Subjected to process ら in which molar o tripled and the tem per alr Vo lume changed 400 k. 300 to
Given that K, for HCIO is 4.0 x 10 8 at 25 °C, what is the value of K, for CIO¯ at 25 °C? Kp %3D Given that Kb for CH,CH,NH, is 6.3 × 104 at 25 °C, what is the value of K, for CH, CH, NH; at 25 °C? K about us privacy policy terms of use contact ushe'p careers 10:39 P 3/10/20 de
Dalton's law states that in a mixture of chemically non-interacting gases, thethe pressure exerted by each contributor at a certain temperature is the same as if it were alone in thein the container alone, and that the total pressure is equal to the sum of the partial pressures(1) of each gas. Deduce this law by kinetic theory from equation 18.11. (1)The partial pressure of a gas in a mixture of ideal gases corresponds to the pressure it would exert if it werealone, occupying the whole container, at the same temperature of the ideal mixture. P = F/A = N*m*Vx^2/V (18.11)
Why is it 2x^2 instead of just 2x ?
Suggest the pressure and temperature at which 1.0 mol of (i) H2O (ii) CO2, (iii) Ar will be in states that correspond to 1.0 mol N2 at 1.0 atm and 25 °C.
(b) Bn MezSiO., MezSiO,, Ме -78 °C, CH2C12 MeO CHO MeO ОН
From the following data determined at 298 K, determine (a) A, H and A₁U for reaction (4) at 298 K; (b) AfH for HI(g) and H₂O(g) at 298 K. Assume ideal gas behavior when necessary. (1) H₂(g) + I2(g) → 2 HI(g) (2) 2H₂(g) + O₂(g) → 2H₂O (g) (3) 1₂ (s)→ I2(g) (4) 4HI(g) + O₂(g) → 21₂(g) + 2H₂O(g) ΔΗΘ = +52.96 kJ mol-¹ A₂H = -483.64 kJ mol-1 A₂H = +62.44 kJ mol-¹
. The equilibrium constant of a gas-phase reaction increasesas temperature is increased. When the nonreacting gasneon is admitted to a mixture of reacting gases (holdingthe temperature and the total pressure fixed and increasing the volume of the reaction vessel), the product yield isobserved to decrease.(a) Is the reaction exothermic or endothermic?(b) Is there a net increase or a net decrease in the number of gas molecules in the reaction?

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