Chemistry help!!! Not sure how to go about solving this...?
2018-05-13 7:04 am
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 x 104 K and a y-intercept of -14.51. Determine the value of ΔH° for this reaction.
回答 (2)
2018-05-13 7:27 pm
One of the forms of Arrhenius equation :
ln(K) = (ΔH/R)(1/T) + ln(A)
As Ea/R and ln(A) are constant, the plot of ln(K) versus 1/T is a linear equation with slope Eₐ/R and y-intercept ln(A).
Slope :
ΔH/R = 1.352 × 10⁴ K
ΔH/[8.314 J/(mol K)] = 1.352 × 10⁴ K
ΔH = (1.352 × 10⁴) × 8.314 J/mol = 1.124 × 10⁵ J/mol = 112.4 kJ/mol
(The given y-intercept is redundant.)
ln(K) = (ΔH/R)(1/T) + ln(A)
As Ea/R and ln(A) are constant, the plot of ln(K) versus 1/T is a linear equation with slope Eₐ/R and y-intercept ln(A).
Slope :
ΔH/R = 1.352 × 10⁴ K
ΔH/[8.314 J/(mol K)] = 1.352 × 10⁴ K
ΔH = (1.352 × 10⁴) × 8.314 J/mol = 1.124 × 10⁵ J/mol = 112.4 kJ/mol
(The given y-intercept is redundant.)
2018-05-14 12:36 am
The value of the y-intercept is 'ln(-14.51)
Antilog
e^(-14.51) = 4.99 x 10^-7
Antilog
e^(-14.51) = 4.99 x 10^-7
收錄日期: 2021-05-01 22:24:59
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