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(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T+0.5 x 10³T² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 105T-² Cp(HCI)/JK¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.

(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T+0.5 x 10³T² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 105T-² Cp(HCI)/JK¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
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(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol¹. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T +0.5 x 10³T ² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 10³T-² Cp(HCI)/JK ¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.
Transcribed Image Text:(ii) The standard enthalpy of formation of HCI(g) at 298 K is equal to -93.2 kJmol¹. Calculate the value of this quantity at 1000 K. Molar heat capacities in this temperature range are given by the empirical equations: Cp(H₂)/JK¹mol¹ = 27.28 +3.25 x 10³T +0.5 x 10³T ² Cp(Cl₂)/JK ¹mol¹ = 36.90 +0.25 x 10³T -2.84 x 10³T-² Cp(HCI)/JK ¹mol¹ = 26.53 +4.60 x 10³T + 1.09 x 105T-² Where T is the thermodynamic temperature.
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