0.100 M AgNO3 50.0 mL 0.100 M HCl 50.0 mL 22.30 23.11℃

0.100 M AgNO3 50.0 mL 0.100 M HCl 50.0 mL 22.30 23.11℃

 

 

When 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl

are mixed in a constant-pressure calorimeter,

the temperature of the mixture increases from 22.30 to 23.11℃.

 

The temperature increase is caused by the following reaction:

AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq)

 

Calculate ΔH for this reaction in kJ/mol AgNO3, assuming

that the combined solution has a mass of 100.0 g

and a specific heat of 4.18 J/g•℃.

 

---------------------------------------------------

 

q = C m Δt

( 참고 https://ywpop.tistory.com/2897 )

 

= (4.18) (100.0) (23.11 – 22.30)

= 338.58 J

 

 

 

(0.100 mol/L) × (50.0/1000 L) = 0.00500 mol AgNO3

( 참고 https://ywpop.tistory.com/7787 )

 

 

 

338.58 J / 0.00500 mol = 67716 J/mol

= 67.7 kJ/mol

---> 1몰당 반응열

 

 

 

발열 반응이므로,

( 22.30 → 23.11℃ )

 

답: ΔH = –67.7 kJ/mol

 

 

 

 

[ 관련 예제 https://ywpop.tistory.com/21183 ] 0.100 M AgNO3 50.0 mL 0.100 M HCl 50.0 mL 22.60℃ 23.40℃

 

 

 

[FAQ] [①23/01/04]