Cu2O(s)의 ΔH°_f = –168.6 kJ/mol, CuO(s)의 ΔH°_f?

Cu2O(s)의 ΔH°_f = –168.6 kJ/mol, CuO(s)의 ΔH°_f?

ΔH°_rxn –146.0 kJ Cu2O(s) ΔH°_f –168.6 kJ/mol CuO(s)

 

 

Copper(I) oxide is oxidized to copper(II) oxide according to the following equation:

Cu2O(s) + 1/2 O2(g) → 2CuO(s) ... ΔH°_rxn = -146.0 kJ

Given that ΔH°_f of Cu2O(s) = -168.6 kJ/mol,

what is ΔH°_f of CuO(s)?

 

 

Given the enthalpy of formation of Cu2O(s) is –168.6 kJ/mol,

calculate the ΔH°_formation of CuO(s) (in kJ/mol).

 

 

Cu2O(s)의 ΔH°_f가 –168.6 kJ/mol이라면,

CuO(s)의 ΔH°_f는 얼마인가?

 

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ΔH°_rxn = [생성물들의 ΔH°_f 합] – [반응물들의 ΔH°_f 합]

( 참고 https://ywpop.tistory.com/3431 )

 

 

 

CuO(s)의 ΔH°_f를 x라 두면,

-146.0 = [2(x)] - [1(–168.6) + 1/2(0)]

 

x = [(–168.6) - 146.0] / 2

= -157.3

 

 

 

답: -157.3 kJ/mol