2HNO3 (1) + 6HB1(g) 4H2O(1) + 2NO(g) + 3B12 (1)Standard Entropies at 25°C (J/mol K)HBr(g)198.6Br2 (1)HNO3 (1)152.2155.6NO(g)210.7H2O(1)69.9ASJ/K3C12 (g) + 3H2O(1) → 5C1¯(ag) + Cl03 (aq) + 6H* (ag)Standard Entropies at 25°C (J/mol·K)Cl2 (9)Cl03 (ag)CI (ag)H* (ag)H,O(1)223.0162.356.50.069.9AS° =J/K2MNO4 (ag) + 6I (ag) + 8H* (ag) 312 (s) + 2MnO2(s) + 4H2O(1)Standard Entropies at 25°C (J/mol K)I (ag)111.3I2 (8)116.1MnO4 (aq)191.2MnO2 (s)53.0H* (ag)0.0H2O(1)69.9AS°J/K

We will calculate ∆S reaction

Standard Entropies at 25°C (J/mol·K) HBr(g) 198.6 Br2 (1) 152.2 HNO3 (1) 155.6 NO(g) 210.7 H2O(1) 69.9 AS J/K %3D 3C12 (9) + 3H2O(1) → 5C1¯(ag) + C1O3 (aq) + 6H* (aq) Standard Entropies at 25°C (J/mol·K) Cl2 (9) Cl03 (ag) Cl (ag) H* (ag) H2O(1) 223.0 162.3 56.5 0.0 69.9 AS J/K %3D 2MNO4 (ag) + 6I (aq) + 8H+ (ag) 312 (s) + 2MNO2 (s) + 4H20(i

Standard Entropies at 25°C (J/mol·K) HBr(g) 198.6 Br2 (1) 152.2 HNO3 (1) 155.6 NO(g) 210.7 H2O(1) 69.9 AS J/K %3D 3C12 (9) + 3H2O(1) → 5C1¯(ag) + C1O3 (aq) + 6H* (aq) Standard Entropies at 25°C (J/mol·K) Cl2 (9) Cl03 (ag) Cl (ag) H* (ag) H2O(1) 223.0 162.3 56.5 0.0 69.9 AS J/K %3D 2MNO4 (ag) + 6I (aq) + 8H+ (ag) 312 (s) + 2MNO2 (s) + 4H20(i

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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A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g•°C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.
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using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔHsoln. Was the dissolution of this salt exothermic or endothermic?
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A B C Cl₂(g) + H₂O(1) HOCI(aq) + HCl(aq) NH₂Cl(aq) + NH4Cl(aq) = 2NH3(aq) + Cl₂(g) CO₂(g) + H₂(g) = H₂O(l) + CO(g) In which of the processes is AH Low (delta is negative). B only A and C only B and C only A, B and C
Determine the boiling point of CS2, in °C, from the following data: CS2(g) CS2(l) ΔHf° / (kJ mol–1) 115.3 87.9 S° / (J mol–1 K–1) 237.8 151.0 Answer Options: 258 -14 116 78 43