(c)For reaction 1 taking place at 120 °C:Hg0(s) + S02(g)= Hg(1) + SO3(g)Reaction 1AreactG® = -13.6 kJ mol-1%3D(i) Given the standard Gibbs free energy above for reaction 1, calculate AreactG when the partialpressures for S0, and SO2 are 1 bar and 0.004, respectively.(ii) Calculate the equilibrium constant for the reaction and hence state what will be the molefraction of SO3 in the gas phase at equilibrium.Note: In calculation assume K=÷; where the term x is the mole fraction of SO3.1-x

Thermodynamics is the branch of chemistry which deals with the study of heat and other forms of…

(c) For reaction 1 taking place at 120 °C: Hg0(s) + SO2(g)= Hg(1) + SO3(g) Reaction 1 AreactG® = -13.6 kJ mol-1 %3D (i) Given the standard Gibbs free energy above for reaction 1, calculate AreactG when the partial pressures for S03 and S02 are 1 bar and 0.004, respectively.

(c) For reaction 1 taking place at 120 °C: Hg0(s) + SO2(g)= Hg(1) + SO3(g) Reaction 1 AreactG® = -13.6 kJ mol-1 %3D (i) Given the standard Gibbs free energy above for reaction 1, calculate AreactG when the partial pressures for S03 and S02 are 1 bar and 0.004, respectively.

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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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

(c)
For reaction 1 taking place at 120 °C:
Hg0(s) + S02(g)= Hg(1) + SO3(g)
Reaction 1
AreactG® = -13.6 kJ mol-1
%3D
(i) Given the standard Gibbs free energy above for reaction 1, calculate AreactG when the partial
pressures for S0, and SO2 are 1 bar and 0.004, respectively.
(ii) Calculate the equilibrium constant for the reaction and hence state what will be the mole
fraction of SO3 in the gas phase at equilibrium.
Note: In calculation assume K=÷; where the term x is the mole fraction of SO3.
1-x

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When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…
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