C+½ 020l co CO (s) 2 (g) CO+ 2 02(a) (g) AH = - 111 kJ %3D CO, 2 (g) Is this reaction endothermic or exothermic? (g) AH = - 394 kJ %3D -11 K3+(-394 C6st O2 (9)-yCO26) AH=-505 KJ Exothermic 2. a) Explain how AT would be affected if a greater amount of surrounding solvent (water) is used, assuming the mass of salt remains constant? b) Explain how qien would be affected if a greater amount of surrounding solvent (water) is used? Explain. If the following enthalpies are known: AH = - 95KJ 2 C+D A+2B- C) AH = + 50kJ B+X

C+½ 020l co CO (s) 2 (g) CO+ 2 02(a) (g) AH = - 111 kJ %3D CO, 2 (g) Is this reaction endothermic or exothermic? (g) AH = - 394 kJ %3D -11 K3+(-394 C6st O2 (9)-yCO26) AH=-505 KJ Exothermic 2. a) Explain how AT would be affected if a greater amount of surrounding solvent (water) is used, assuming the mass of salt remains constant? b) Explain how qien would be affected if a greater amount of surrounding solvent (water) is used? Explain. If the following enthalpies are known: AH = - 95KJ 2 C+D A+2B- C) AH = + 50kJ B+X

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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The element chlorine is a useful reagent. For example, it is used for the production of phosgene (carbonyl chloride) from gaseous carbon monoxide CO(g) + Cl2(g) → COCl2(g) Substance COCl2(g) CO(g) Cl2(g) AH (hJL) kJ mol AS (mol·K J - 219.1 283.5 - 110.5 000.0 197.7 223.1 This reaction will be spontaneous at temperatures lower than:
Consider the equilibrium reaction shown below: Cu (s) + 3 NO31 (aq) + 8 H*' (aq) 4 3 Cu+2 (aq) + 2 NO (g) + 4 H20 (1) What is the Kc for this reaction? Select one: [Cu*2j*[NO]? [NO,'j°[H+1j® O a. K. [Cu*2j®[NO}°[H,Of* [NO,'j°[H+lj*[Cu] O b. K. = [Cu+2]°+[NO]? [H**j® [NO,'j³+ O c. Ke = [NO,'j*[H+1j$ [Cu+2]°[NO]? O d. K. = e. К. [Cu][NO;'j°[H *+1]® Kc е. (Cut2]°[NO]°[H2O}*
Use the following information to calculate the standard enthalpy of formation of NO>(g) at 298 K? N2(g)+ O2(g) - 2NO(g) AH =180.5 kJ 298 NO2(g) - % O2(g) + NO(g) AHOR =57.06 kJ
A process of synthesizing NH3 through the reaction: 3H (g) + N (g) 2 2NH (g) AG°(NH ) 16500J (pada 25ºC) mol AH reaction = -92.400 J/mol. Ammonia synthesis is difficult to carry out although thermodynamically the process can take place spontaneously. a) Explain why ammonia is difficult to produce on an industrial scale? b) What is the solution so that ammonia synthesis can run quickly so that it is profitable if it is produced on an industrial scale?
1. Calculate the AHrxn for the reaction, Sn (s) + Cl2 (g) SNC12 (s) AHrxn = ? Sn (s) + Cl2 (g) → SnCl2 (s) Sn (s) + 2C12 (g) → SnClą (1); AH = – 545.2 kJ SNC12 (s) + Cl2 (g) Eq. 1 Eq.2 Eq.3 SnCl4 (1); AH = – 195.4 kJ
Which of the following processes yields a AS = - ? O2 NO(g) + O2(g) ---> 2 NO2(g) NaCIO3(s)---> Na (aq) + CIO3(aq) COCI2(g) -- CO(g) + Cl2(g) CH3OH(1) ---> CO(g) + 2H2(g) None HII>
Please provide neat solution
4 (a) Calculate the value of Kc for the reaction: PCl5 (g) PCl3 (g) + Cl2 (g) ΔH = Positive Given that when 8.4 mol of PCl5 (g) is mixed with 1.8 mol of PCl3 (g) and allowed to come to equilibrium in a 10 dm3 container the amount of PCl5 (g) at equilibrium is 7.2 mol. Kc = (b) Explain the effect of the following changes below on the value of Kc: Increasing temperature Lowering the concentration of chlorine (Cl2) Addition of a catalyst
Calculate the standard free energy change for the reaction below. N2(g) + 3H2(g) → 2NH3(g) given that the standard free energy of formation [AG%] of the product is -26.2 kJ/mol. (3) +26.2 kJ/mol (2) +8.40 kJ/mol (4) -26.2 kJ/mol O (1) -52.4 kJ/mol L A Moving to the next question prevents changes to this answer. MacBook Pro
Is the reaction endothermic or exothermic?
Find the AH of the following reaction: 2NOCI(g) given the following reactions: N;(g) + }0,(g) NO(g) + ¿Cl,(g) N2(g) + O2(g) + Cl½(g) NO(g) AH = 98.6 kJ NOCI(g) AH =- 36.8 kJ
Given the reactions, X(s) + 1/2O₂(g) XCO₂ (s) XO(s) XO(s) + CO₂(g) what is AH for this reaction? X(s) + 1/2O₂(g) + CO₂(g) AH = -763.1 kJ AH = +159.3 kJ XCO3(s)