uestion 27 DSe(s) +3 F2(g) → SeF6(g)AS' = -337 J/(mol,n· K)SubstanceApproximateS (J/(mol · K))Se(s)42F2(g)SeF6(g)314The chemical equation above represents the formation of SeFe(9) from its elements and the table provides the approximate values of S for Se(s) and SEF6(g). Based on the data, which of the followingmathematical expressions can be used to correctly calculate S" for F2(g) ?S = [- 337 + 314 – 42) J/(mol K)S = -- 337- 314 + 42 J/(mol K)S = - 337 +314 - 42) J/(mol - K)S =-- 337 - 314 + 42 J/(mol - K)D.escQ Search or enter website name$%&#

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Chemistry

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

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Chapter1: Chemical Foundations

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

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A chemist measures the energy change AH during the following reaction: 2 Fe₂O3(s) 4 FeO(s) + O₂(g) 1 AH 560, kJ Use the information to answer the following questions. This reaction is... Suppose 25.9 g of Fe₂O3 react. Will any heat be released or absorbed? If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Be sure your answer has the correct number of significant digits. endothermic exothermic OYes, absorbed. Yes, released. No. 0... X G
In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe,O3(s) + 3CO(g) 2Fe(s) + 3CO,(g) AH° = - 28 kJ 3Fc,O3() + CO(g) 2Fe3O4() + CO,(g) AH = -59 kJ FezO4(s) + CO(g) 3FcO(s) + CO,(g) AH° = +38 kJ to calculate AH° for the reaction FeO() + CO(g) Fe(s) + CO2(g) AH° = i kJ
How many kilojoules of energy are generated when in 82.8 grams of CO(g) reacts according to the following reaction? CO(g) + O2 (g) → CO2(9) Hint: balance the reaction first Answer in decimal form with 1 decimal place Compound H; (KJ/mol) Compound H;(KJ/mol) CH(9) HCl(g) H,0(g) H2O(1) H2 S(g) 89.5 H2SO,(1) 33 M9SO, (s) -75.7 -93.2 Co2(9) 394.4 -242.7 SO2 (g) NH,C(s) NO(g) NO,(g) -297 -286.7 -316.3 -21 -812.2 -1279.1 SnCl4 (1) Sn0(s) SnO2(s) NaF(s) NaOH(s) Mn0(s) :-287.1 MnO2(s) -581.6 NaCl(s) SO: (9) Zn0(s) ZnS(s) -546.1 -385.8 -520.0 -411.9 -569.9 -396.1 -427.6 -3489 NH3 (9) -47.1 -203.8 CO(g) -111.4 O2(9)
A chemist measures the energy change AH during the following reaction: 2 Fe,03(5) → 4 Fe(5)+O,(g) AH=560. kJ Use the information to answer the following question. Suppose 49.9 g of Fe,0, react. Calculate how much heat will be released or absorbed. ? Round your answer to 3 significant digits.
Using Hess's law, what is AHf rxn for the following reaction? NO(G) + O(g) – NO2(9) NO(g) + O3(9) – NO2(9) +O2(9) AH xn = -198.8 kJ/mol Og(9) – 3/2 02(9) AHrxn = -142.2 kJ/mol 02(9) → 20(9) AH Prxn = +498.8 kJ/mol -839.8 kJ/mol -306.0 kJ/mol 394.9 kJ/mol 157.9 kJ/mol O 442.3 kJ/mol QUESTION 8 Octane (C3H18) undergoes combustion according to the following thermochemical equation. 2C8H18() + 2502(g) – 16CO2(g) + 18H20() AH°rxn = -1.0940 x 104KJ/mol What is the standard enthalpy of formation of liquid octane? AH°{(CO2(g)) = -393.5 kJ/mol and AH°F{H2O(1)) = -285.8 kJ/mol 495 kl/mol O -250 kJ/mol -495 kJ/mol -10,940. kJ/mol -2188 kJ/mol
A chemist measures the energy change AH during the following reaction: 2 NH;(g) - N(9)+3H,(9) AH=160, kJ Use the information to answer the following questions. O endothermic. This reaction is... O exothermic. Suppose 93.6 g of NH, react. O Yes, absorbed. O Yes, released. Will any heat be released or absorbed? O No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. Explanation Check 02021 McGraw Hill LLC. Al Rights Reserved Terms of Use Pivecy
When HCI(g) reacts with O₂(g) according to the following reaction, 28.6 kJ of energy are evolved for each mole of HCI(g) that reacts. Complete the following thermochemical equation. 4HCI(g) + O₂(g)2H₂O(g) + 2Cl₂(g) ΔΗ = 28.6| kj
The following thermochemical equation is for the reaction of Fe3O4(s) with hydrogen (g) to form iron(s) and water(g). Fe3O4(s) + 4H₂(g) 3Fe(s) + 4H₂O(g) ΔΗ = 151 kJ When 81.5 grams of Fe3O4(s) react with excess hydrogen (g), kJ of energy are 0. Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.
The combustion of a sample of isoctane vapor at constant pressure raises the temperature of a calorimeter and its contents by 0.400 °C. The heat capacity of the calorimeter and water combined is 2.48 kJ/°C. How much heat was produced from the combustion? (variations of formula: c=q/mat)
A scientist measures the standard enthalpy change for the following reaction to be 184.8 kJ:Fe3O4(s) + 4 H2(g) 3Fe(s) + 4 H2O(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Fe3O4(s) is kJ/mol.
Using the provided table and the equation below, determine the heat of formation (in kJ/mol) for PbS. 2 PbS (s) + 3 O₂ (g) → 2 SO₂ (g) + 2 PbO (s) AH° = -828.4 kJ/mol Substance O₂ (g) SO: (g) PbO (S) AHf (kJ/mol) 0 -296.9 -217.3
Sulfur dioxide, SO, (g), can react with oxygen to produce sulfur trioxide, SO, (g), by the reaction 2 SO, (g) + 0,(g) → 2 SO,(g) The standard enthalpies of formation for SO,(g) and SO, (g) are AH; [SO,() = -296.8 kJ/mol AH; SO,( = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 4.10 L of SO, (g) is converted to 4.10 L of SO, (g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior. kJ AL = 18.249 incbrcect

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