What is the equilibrium constant at 1000 K for the reaction shown below if its AG° at 1000 K is 32 kJ/mol?N2(9) + C2H2(g)→ 2 HCN9)1.0O47O 3.8O 0.021Calculate the total heat required in the heating and complete melting of 1.00 mol solid Cu (MM = 63.55 g/mol) from 100.0 °C to its normal melting point of 1085.0°C.Given:AHfus = 13.1 kJ/molCp of Cus) = 24.47 J/mol-°C%3DCp of Cu = 36.33 J/mol-°CO24.1 kJO 37.2 kJO 48.9 kJO 39.6 kJCorrosion of Fe to its oxides (e.g. FeO, Fe203) in moist air is an example of a spontaneous process with negative AG and which requires no added work for thereaction to proceed forward.Select one:O TrueO False

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What is the equilibrium constant at 1000 K for the reaction shown below if its AG at 1000 K is 32 kJ/mol? N2(9) + C2H2(g) → 2 HCN(9) O 1.0 O 47 O 3.8 O 0.021

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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Question

What is the equilibrium constant at 1000 K for the reaction shown below if its AG° at 1000 K is 32 kJ/mol?
N2(9) + C2H2(g)→ 2 HCN9)
1.0
O47
O 3.8
O 0.021
Calculate the total heat required in the heating and complete melting of 1.00 mol solid Cu (MM = 63.55 g/mol) from 100.0 °C to its normal melting point of 1085.0
°C.
Given:
AHfus = 13.1 kJ/mol
Cp of Cus) = 24.47 J/mol-°C
%3D
Cp of Cu = 36.33 J/mol-°C
O24.1 kJ
O 37.2 kJ
O 48.9 kJ
O 39.6 kJ
Corrosion of Fe to its oxides (e.g. FeO, Fe203) in moist air is an example of a spontaneous process with negative AG and which requires no added work for the
reaction to proceed forward.
Select one:
O True
O False

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