EXERSICE 1 An ideal gas undergoes a process A -> B in two alternative ways: i) reversible and ii) irreversible. Which of the following options are always correct? Provide a brief and sufficient justification for your selections and exclusions. The symbol S refers to the ideal gas System unless the Universe is explicitly referred to as the Suniverse. ASrev. = 0 ASirrev>0 AS Suniverse |rev = 0 ASuniverse rev <0 Suniverse irrey > 0 ASaçx.

EXERSICE 1 An ideal gas undergoes a process A -> B in two alternative ways: i) reversible and ii) irreversible. Which of the following options are always correct? Provide a brief and sufficient justification for your selections and exclusions. The symbol S refers to the ideal gas System unless the Universe is explicitly referred to as the Suniverse. ASrev. = 0 ASirrev>0 AS Suniverse |rev = 0 ASuniverse rev <0 Suniverse irrey > 0 ASaçx.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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5. One mole of a monatomic ideal gas is compressed adiabatically in a single stage with a constant opposing pressure equal to 10 atm. Initially the gas is at 27 °C and 1 atm pressure, the final pressure is 10 atm. How would the various quantities be affected if n moles were used instead of one mole? For a monatomic ideal gas. C₂ = Cv R. 2
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Hess's Law II Calculate A,H for the reaction, from the following information: 2 Ni(s) + 1/4 Sg(s) + 3 O₂(g) ----> 2 NISO3(s) NISO3(s) ----> NiO(s) + SO₂(9) 1/8 Sg(s) + O₂(g) ----> SO₂(g) Ni(s) + 1/2O₂(g) ----> NiO(s) AH 166.00 kJ AH = -247.00 kJ A,H= -251.00 kJ
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Consider a gas obeying van der waals equation. Let one mole of the gas expands reversibly from volume ΔΗ, under isothermal condition. The expression of ORT 1 1 V ·b V -b m2 m1 bRT a V m2 1 Vm2-b V V ORT In- m1 V -b m2 V-b m1 1 m1 V b -b m for this process is: a m2 + 2a V m2 a V + m1 2a V. m1 V V m1 to m2
3. Heats of reaction can also be calculated using heats of formation and the relationship - AHrxn = ΣnAHƒ.prod — ΣmAHƒ.reac Substance HCl(aq) MgCl2(aq) MgO(s) H₂O(/) H.(kJ/mol) -167.2 -796.8 -601.2 -285.8 0 a. Standard State Elements Calculate the theoretical AH° values for the following reaction Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) Mg(s) + O2(g) → MgO(s)
Initially at 300 K and 10 atm pressure, 1 mol of a gas is allowed to expand adiabatically against a constant pressure of 4 atm until equilibrium is achieved. Assume the gas to be ideal with Cp,m = 28.58 + 1.76 x 10^-2 T(The units of T are K and the units of Cp,m are J K-1 mol-1.) Compute DU, DH, q and w.
In which of the following processes is AH = AU? Two moles of hydrogen iodide gas react to form hydrogen gas and iodine gas in a 40-L container. O Calcium carbonate is heated to form calcium oxide and carbon dioxide in a container with variable volume. One mole of solid carbon dioxide sublimes to the gas phase. O One gram of water is vaporized at 100°C and 1 atm. O Two moles of ammonia gas are cooled from 325°C to 300°C at 1.2 atm
CaCO3(s)⇄CaO(s)+CO2(g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0mol sample of CaCO3(s) is placed in a rigid 100.L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00atm, while some CaCO3(s) remains in the vessel. (a) Calculate the number of moles of CO2(g) present in the vessel at equilibrium. (b) Write the expression for Kp, the equilibrium constant for the reaction, and determine its value at 898°C. (c) The experiment was repeated, but this time starting with a 4.0mol sample of CaCO3(s). On the following graph, draw a curve showing how the pressure of CO2(g) would change over time as the vessel is heated to 898°C and equilibrium is established.
A student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.
1.00 mole of an ideal diatomic gas (for which Cv 5R/2) is in a rigid container with a constant volume of 2.00 L. The gas is heated from 250.0 K to 300.0 K. Calculate the AS(gas) for this process, in J/K. J/K 1 4 C 7 8 +/- x 10 3. co 2. 5,